H2 (g) + I2 (g) yields (k1 on top of the arrow) 2HI (g) (one step reaction)Mechanism b. Unlock. Hydrogen iodide decomposes according to the equation 2HI(g) H2(g) + I2(g), for which Kc = 0. Chemistry. What is the reaction quotient, Q, for this system when [H2] = 0. Question: At 500 °C, hydrogen iodide decomposes according to 2HI(g)↽−−⇀H2(g)+I2(g) For HI(g) heated to 500 °C in a 1. In another study of the formation of HI(g), H2(g) and I2(g) were placed in a sealed container at a certain temperature. What will be the concentration of HI after t = 1.414 M, L) = 0.300 mol of I2 were placed in a 1. 0. 2HI(g)⇌H2(g)+I2(g) Kc=[H2]/[I2][HI]^2.B.06 M The equilibrium constant, K c, for the reaction H2 (g) + I2 (g) ⇄ 2HI (g) at 425°C.200 atm, and a partial pressure of HI of 0. The equilibrium constant Kc for the reaction H2 (g) + I2 (g) <=> 2 HI (g) is 54. What is the value of Keq for the equilibrium below? 1/2H₂ (g) + 1/2 I₂ (g) ⇌ HI (g), The value of Keq for the equilibrium H₂ (g) + I₂ (g) ⇌ 2 HI (g) is 794 at 25°C. Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H.60 mol/L, [H2] = 0.00 L vessel at 698 K.15 M I2 at equilibrium.550 mol HI was injected into a 2.2. Show below how to derive the Keq .15) (15.0 H―I 298.016 Initially a container contains 0. roughly equal amounts of products and reactants are present d. 2) Suppose a reaction is started with 0. Chemistry questions and answers.0 = cK ?C°354 ta enidoi dna ,negordyh ,edidoi negordyh neewteb muirbiliuqe eht rof ,)Jk( °GΔ ,egnahc ygrene eerf eht si tahW :noitseuQ .0 M HI is placed into a closed container and the reaction is allowed to reach equilibrium at 25∘C, what is the equilibrium concentration of H2 (g)? Question: Consider the second-order reaction: 2HI(g) →H2(g) + I2(g) Use the simulation to find the initial concentration (HI), and the rate constant k for the reaction. Iodine is in Group VIIA, so it has an oxidation number of -1 in both the reactant I2 and product HI. C. Chemistry questions and answers.94×10-2 at 728 K.0 g of l2 (g). What is the equilibrium concentration of H2? 2)For the reaction: 2HBr (g) ↔ H2 (g) + Br2 (g) Initially a container contains 0.80×10-2 at 698 K. (Express your answer using two H2 (g) +I2 (g) <-----> 2HI (g) At equilibrium in a particular experiment, the concentrations of H2,I2 , and HI were 0. The equilibrium constant (Kc) for the reaction H2 (g) + I2 (g) <=> 2HI (g) is 54.040. Since there is an equal number of each element in the reactants and products of H2 + I2 = 2HI, the equation is balanced.95M.0 minutes? 1 pts.015 2HI (g) [image] H2 (g) + I2 (g) 6 kJ 9 kJ 15 kJ 20 kJ 22 kJ. Qc=[HI][H2][I2] There are 2 steps to solve this one. Russia said it had suppressed a drone attack on Moscow carried out by Ukraine which it has accused of "international terrorism.550 M b.10 x 10^-5 L/mol*s at 600 K. The equilibrium constant, K c, for the reaction H 2 ( g) + I 2 ( g) ⇄ 2HI ( g) at 425°C is 54. What will be the concentration of HI after t = 4.16 M and their equilibrium concentrations are both 0. [2] The equilibrium will shift to the right. The equilibrium constant, Kc, for the following reaction is 1. See Answer Chemistry Chemistry questions and answers Hydrogen iodide decomposes according to the equation 2HI (g) H2 (g) + I2 (g), for which Kc = 0.00-L reaction The equilibrium constant for the gas phase reaction H2 (g) + I2 (g) 2HI (g) is Keq = 50 at 25 °C. loading. Chemistry questions and answers. If the initial concentration of HI is 4.76×1010 s ([HI]t) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. where K K is the equilibrium constant expressed in units of concentration and Δn Δ n is the difference … \[\ce{H2(g) + I2(g) \rightleftharpoons 2HI(g)} + \text{heat} \label{15.Ea = - (8.3.0049. Calculate Kc for the reaction 2HI(g) = H2(g) + I2(g) given that the concentration of each species at equilibrium are as follows: [HI] = 0. This is because the reaction is exothermic and releases heat.1 x 10-2 M, how many minutes will it take for the concentration to. 2HI(g) > H2(g) + I2(g) Calculate Kc at this temperature for: H2(g) + I2(g) 2HI(g) Kc= 2.200 mol H2 and 0.85 mol/L, [I2] = 0. About us. Expert Answer.52 x 10-7 L/mols.984 mole of I2, and 0.550 mol HI was injected into a 2. ΔG°, for the reaction shown below at 453°C? 2HI(g) ↔ H2(g) + I2(g) Kp = 0.59×10 −3 MM , [H2]=[H2]= 4. 1 Answer Stefan V.393 M. In a certain experiment the decomposition of hydrogen iodide on finely divided gold is zeroth order with respect to HI.5 k J/m o l r x n H 2 (g) and I 2 (g) can react to produce HI (g) , as represented above. What concentration of HI is present at equilibrium? 2HI (g) -> H2 (g) + I2 (g) There are 2 Hydrogen atoms and 2 Iodine atoms on the right so the have to be 2 of each on the left as well, so there are 2 HI molecules on the left. The equilibrium constant, Kp, is related to the standard Gibbs free energy change, ΔG°, through the equation: Find Kc for the reaction.60 kJ/mol.4 kg of CO 2 at 825 K. Express your answer using two significant figures. Nhận xét nào sau đây không đúng? A.815 atm 2. The potential energy of the reactants is indicated on the diagram.50 M? 613. For the following systems at equilibrium A:B:2NOCl (g)H2 (g)+I2 (g)⇌⇌2NO (g)+Cl2 (g)2HI (g)A:2NOCl (g)⇌2NO (g)+Cl2 (g)B:H2 (g)+I2 (g)⇌2HI (g) classify these changes by their effect. CH 4 (g) + CO 2 (g) ⇌ 2CO(g) + 2H 2 (g); K p = 450. The equilibrium reaction can be written as follows: 2HI(g) ⇌ H2(g) + I2(g).0013 verified answered • expert verified H 2 (g)+I 2 (g)→2 H I (g) ΔH∘r x n=−9.75M[H2]=3.708 atm, and PH2=P12=0.28×10 10 s ([HI]t) for a reaction starting under the condition in the simulation?.15 K are summarized in Table 4. Chemistry Chemical Equilibrium Equilibrium Constants. How does the magnitude of Kp for the reaction 2HI(g)⇋H2(g)+I2(g) change if the equilibrium is written 6HI(g)⇋3H2(g)+3I2(g)? It is cubed.0 M HI is placed into a closed container and the reaction is allowed to reach equilibrium at 25 ∘C , what is the equilibrium concentration of H2 (g)? a 0 H2 (g)+I2 (g)→2HI (g) ΔH∘rxn=−9.90×1010 s ( [HI]t) for a reaction starting under the condition in the simulation? Chemistry questions and answers. At this temperature, what is the value.65 x 10-2 mol-1 L s-1. If the initial concentration of HI in a container is 5. 2SO3(g) > 2SO2(g) + O2(g) Calculate Kc at this temperature for the following reaction: SO3(g H2, I2, and HI are introduced into a flask.70 M0.036. 1, 2023.00 L reaction vessel at 400ºC. At this temperature, what is the value.1 a otni decudortni era IH fo selom 323. where K K is the equilibrium constant expressed in units of concentration and Δn Δ n is the difference between the numbers of moles of gaseous products and gaseous reactants ( np −nr n p − n r ). Therefore, in the reaction H₂(g) + I₂(g) → 2HI(g), both hydrogen and iodine change their oxidation states: Hydrogen from 0 to +1 and Iodine from 0 to -1. Answer: Increasing the temperature will cause the equilibrium to shift towards the reactants (left).80M.2.50 at 400∘C (b) H2( g)+I2( g) ⇌ 2HI(g) Kc = 50.484 M , and [HI]=4. H2(g)+I2(g)=2HI, Finding out final concentration of H2, I2 an… Balanced Chemical Equation 2 HI → H 2 + I 2 ⬇ Scroll down to see reaction info and a step-by-step answer, or balance another equation. At equilibrium, pH2= 1.The amount of I2 produced over time is measured by opening each 2HI(g)⇌H2(g)+I2(g)2HI(g)⇌H2(g)+I2(g) At equilibrium it is found that [HI]=[HI]= 3.4 x 10^-9 l/(mol x s) at In an experiment, 0.2 at 448∘C (c) Na2SO4 ⋅ 10H2O (s) ⇌ Na2SO4( s)+ 10H2O (g) KP = 4. 0. This problem has been solved! \[\ce{H2(g) + I2(g) \rightleftharpoons 2HI(g)} + \text{heat} \label{15. … Kp = K(RT)Δn (15.87×10 −4 MM . There are 2 steps to solve this one.2 kcal/mol (−9.0 (c) CO2 (𝑔)+H2 (𝑔) CO (𝑔)+H2O (𝑔) T=980°C 𝐾𝑝=1. View Available Hint (s)for Part A Reset Help System A Increase HI decomposes to H2 and I2 by the following equation: 2HI(g) → H2(g) + I2(g);Kc = 1. The rate constant at 555 K is 3. 0.09 M . A flask originally contains 0. Step 1.00 × 10^−19 at 298 K what can be said about this reaction at this temperature? The equilibrium lies far to the left.50-L container initially holds 0. Of 0.314 J/mol*K) (ln 1. Step 2.75 M H2 and 0. Calculate the equilibrium concentrations of the three gases.30 kJ/mol at 25°C. 25.016 Initially a container contains 0.10x10^-5 L/mol*s / 9.10) with K varying between 1.51 x 10^-9 L/mol*s at 500 K and 1. H2(g) + I2(g) ⇌ 2HI (g) = -9,6 kJ. H2(g) + I2(g) 2HI(g) When equilibrium is achieved the concentration of HI is 0. Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced. For the reaction 2HI (g) ⇌H2 (g)+I2 (g), Kc= 0.0 x 10-4 M? Question: Calculate ΔG° for each of the following reactions from the equilibrium constant at the temperature given.87×10 −4 MM , and [I2]=[I2]= 4., When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the The correct answer is 0. Calculate K for this reaction.0 L reaction container initially contains 22.0200 M . Find Ea. The equilibrium constant for a system will be symbolized by the letter: K.9 g I2.072 M at 430 degree C.2Group of answer choices0.035 C) 28 D) 397 E) 0. Thus an equilibrium mixture of H2, D2, and HD contains significant concentrations of both product and reactants. B) The equilibrium will shift to th; The following reaction is exothermic.51 x 10^-9 L/mol*s at 500 K and 1.83×10−4 M . CO2 g+H2 g⇌CO g+H2O g. (a) N2( g)+ 3H2( g)⇌ 2NH3( g) Kc = 0. Thus, increasing … H2 (g) + I2 (g) → 2HI (g) A student makes the following statements: Hydrogen always has the same oxidation number, so it has an oxidation number of +1 in … H2(g) and I2(g) can react to produce HI(g), as represented above.450 mol/L∙s. Consider the following exothermic reaction: 2HI (g) ⇆ H2 (g) + I2 (g) A) What will happen to the reaction mixture at equilibrium if an inert gas is added? [1] The equilibrium will shift to the left.02×10-2 at 907.0175 mol/L. Chemistry questions and answers. At a certain temperature, the equilibrium constant, Kc for this reaction is 53. Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced.00 mole of HI are introduced into a 1. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature.snib evitcepser rieht ot smeti etairporppa eht garD .550 mol HI is injected into a 2. Part A. Choose the one alternative that best completes the statement or answers the question.1×10−4 (b) H2 (𝑔)+I2 (𝑔) 2HI (𝑔) T=400°C 𝐾𝑝=50.0156 at 400°C 單選: 2. Khi tăng nhiệt độ, cân bằng trên chuyển dịch theo chiều nghịch. Phát biểu nào sau đây về sự trao đổi năng lượng của phản ứng trên là đúng? A.0960 atm. What is the equilibrium concentration of H2? Question: Hydrogen iodide decomposes according to the equation 2HI (g) H2 (g) + I2 (g), for which Kc = 0. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature. Chemistry. 2HI (g) = H2 (g) + I2 (g) Calculate Kc at this temperature for the following reaction: HI (g) =1/2H2 (g) + 1/2I2 (g) 6) a CO2 g+H2 g⇌CO g+H2O g.0890 M HI, 0. At this temperature, what is the value of Keq for the equilibrium You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Calculate the concentration of H2 at equilibrium. Calculate the concentrations of the gases at equilibrium. The equilibrium constant, Kc, for the following reaction is 1.5kJ/molrxn. Similar questions.9 and 4 over a wide temperature range (100-1000 K). Calculate the concentration of HI at equilibrium. Flashcards; Test; Learn Study with Quizlet and memorize flashcards containing terms like The value of Keq for the equilibrium H₂ (g) + I₂ (g) ⇌ 2HI (g) is 794 at 25 °C. An 85. Study with Quizlet and memorize flashcards containing terms like 42) Of the following equilibria, only _____ will shift to the left in response to a decrease in volume. The equilibrium concentration of I2 is 0.25 Consider the reaction: H2 (g) +I2 (g) 2 HI (g) A reaction mixture in a 3. With time, the concentrations of H2 and I2 decline, and the concentration of HI increases.8.2. At this temperature, what is the value of Keq for the equilibrium below? HI (g) ⇌ 1/2 H2 (g) + 1/2 I2 (g) The value of Keq for the equilibrium H2 (g) + I2 (g) 2HI (g) is 794 at 25 °C. Ở nhiệt độ không đổi, khi tăng áp suất thì cân bằng không bị chuyển dịch.. The rate constant at 555 K is 3.21 If at equilibrium the reaction vessel contains 1. 1. What is the free energy change, ΔG°, for the Question.215 M H2, and 0. The law of mass action best fits which of the following descriptions? Find the equilibrium expression for the reversible reaction below. So if you add heat, more N2 (g) and H2 (g) will be created and balance out the reaction.53×1010 s ([HI]t) for a reaction starting under the condition in the simulation? Given from simulation: Rate Law: k[HI]^2 Question. H2(g) + I2(g) → 2HI (g) ∆H = +11,3 kJ. What is the value of Keq for the equilibrium below? 1/2 H2 (g) + 1/2 I2 (g) HI (g) A) 1588 B) 0. The equilibrium constant, Kc, for the following reaction is 1. An additional 0.0 (at 400ºC) If the reaction vessel initially contains 0. H2(g) +D2(g) ⇌ 2HD(g) (15. Step 2. Express your answer using two significant The decomposition of HI (g) is represented by the equation 2HI (g) = H2 (g) + I2 (g) The following experiment was devised to determine the equilibrium constant of the reaction. Assuming all gases are at the same Question: The following reaction was performed in a sealed vessel at 721 ∘C∘C : H2(g)+I2(g)⇌2HI(g)H2(g)+I2(g)⇌2HI(g) Initially, only H2H2 and I2I2 were present at concentrations of [H2]=3. reactants predominate c.708 atm, and PH2 = PI2 = 0.761 g H2 and 96. Consider the following reaction: H2 (g) + I2 (g) ⇌ 2 HI (g) Complete the following table. Q. Consider the equilibrium reaction and its equilibrium constant expression. At this temperature, what is the value of Keq for … The equilibrium concentration of I2 is 0.040; This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.43 atm b! 3.0535 0.040; This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.

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80×10-4 mol L-1 s-1 If the experiment has an initial HI concentration of 0.16 M and their equilibrium concentrations are both 0. H2 (g)+I2 (g)⇌2HI (g) has Δ H =−2. Consider the reaction H2(g) + I2(g) <--> 2HI(g).65 M HBr and no product.15 298.15M and [I2]=2.67 (d) CaCO3 (𝑠) CaO (𝑠)+CO2 At 25°C, the equilibrium constant, Kp, for the reaction H2(g) + I2(g) ⇌ 2HI(g) is approximately 0. Who are the experts? Experts have been vetted by Chegg as specialists in this subject. At this temperature, what is the value of Keq for the equilibrium below? HI (g) ⇋1/2 H2 (g) + 1/2 I2 (g) 2. 21.20 M of H₂ and 1. What is the standard free energy change, ΔG°, for the reaction shown below at 453°C? 2HI(g) ↔ H2(g) + I2(g) Kp = 0.70 atm 13.0156 at 400ºC.55M respectively.4x10^-9 L/mol.42 mol of CO and 0.42 times 10^{-7} L/mol . What is the new partial pressure of HI? H2(g) + I2(g) → 2HI(g) (a) Using the equation ΔH o rxn = ∑(BE(reactants)) − ∑(BE(products)) kJ/mol (b) Using the equation ΔH o rxn = ∑(nΔH o f (products)) − ∑(mΔH o f (reactants)) kJ/mol Bond BE kJ/mol Substance ΔH o f kJ/mol H―H 436. These results can be used to calculate the standard Gibbs free … verified answered • expert verified H 2 (g)+I 2 (g)→2 H I (g) ΔH∘r x n=−9. s.75 M I2, what is the equilibrium concentration of HI? The activation energy for the decomposition of Hi(g) to H2(g) and I2(g) is 186 kJ/mol. Question: 6) a. What will be the concentration of HI after t = 9. 2HI(g) = H2(g) + I2(g) Calculate Kc at this temperature for the following reaction: HI(g) =1/2H2(g) + 1/2I2(g) This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Determine the initial and equilibrium concentrations of HI if the initial concentrations of H2 and I2 are both 0.)The equilibrium constant, Kc, for the following reaction is 1. Expert-verified.4 H2(g) 0 I―I 151 I2(g) 61. Chemistry questions and answers. So, this is indeed a redox reaction because oxidation (the loss of electrons as seen in The equilibrium constant, Kc, for the following reaction is 1. The equilibrium constant for a system will be symbolized by the letter: K.708 atm, PH2 = PI2), we can substitute them into the equilibrium expression for the reaction, which is Kp = (PH2 * PI2) / (PHI)^2. H2 (g) and I2 (g) can react to produce HI (g), as represented above.0300 M .200 atm, a partial pressure of I2 of 0. Question: Consider the equilibrium system involving the decomposition of hydrogen iodide. Consider the reaction H2(g) + I2(g) <--> 2HI(g). Chemistry questions and answers. At this temperature, what is the value of Keq for the equilibrium below? HI (g) ⇌ 1/2 H2 (g) + 1/2 I2 (g) The value of Keq for the equilibrium H2 (g) + I2 (g) 2HI (g) is 794 at 25 °C.9. Chemistry questions and answers.65 M HBr and no product.09 M . please do step by step. freedom in Russia, including a law passed in December against depictions of gay lifestyles — what the government called "gay Investigators examine an area next to a damaged building in the "Moscow City" business district after a reported drone attack in Moscow, Russia, early Tuesday, Aug. Equilibrium concentration of H1 increases 2.6 × 10−3 at 25∘C If 1. Flashcards; Test; Learn Study with Quizlet and memorize flashcards containing terms like The value of Keq for the equilibrium H₂ (g) + I₂ (g) ⇌ 2HI (g) is 794 at 25 °C.498 M I2. Study with Quizlet and memorize flashcards containing terms like If a given process proceeds spontaneously toward the products, the value of the reaction quotient Q is _____ the equilibrium constant K, and ΔG for the reaction will be _____.83×10−4 M , and [I2]= 4. What is the equilibrium concentration of H2? 2)For the reaction: 2HBr (g) ↔ H2 (g) + Br2 (g) Initially a container contains 0.0500 M .038 M H2, and 0.00-L container.35 M0.295. a) Carefully complete the energy diagram by drawing a curve that accurately shows the progress of Question: Consider the following reaction for the decomposition of HI at a certain temperature 2HI(g) --> H2(g) + I2(g) the average rate of disappearance of HI over the period from t = 0 to t = 5. Consider the second-order reaction: 2HI (g)→H2 (g)+I2 (g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. Since there is an equal number of each element in the reactants and products of H2 + I2 = 2HI, the equation is balanced.50 M? [H2] = 0. Question: The decomposition of hydrogen iodide, 2HI (g) ----> 2H2 (g) + I2 (g), has rate constants of 9. Consider the following chemical reaction: CO (g) + 2H2 (g) ⇋CH3OH (g) At equilibrium in a particular experiment, the concentrations of CO Question: Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. About Quizlet; How Quizlet works; Careers; Advertise with us; Get the app; For students. About Quizlet; How Quizlet works; Careers; Advertise with us; Get the app; For students. Explain the concept of a dynamic equilibrium.016 Initially a container contains 0. Balance the The oxidation state of an element in its elementary state, such as H₂ or I₂, is always 0. Ở nhiệt độ không đổi, khi tăng nồng độ H2 hoặc I2 thì You'll get a detailed solution from a subject matter expert that helps you learn core concepts.0156 at 400ºC. In a 2. Suggest Corrections.0 atm.00 mole of H2, 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2]=0. The equilibrium constant, Kc, for the following reaction is 1. The reaction rate is a direct function of the reactants concentrations, aA+ bB → cC #"Rate" = k[A]^x [B]^y# Where #a, b, c#: are the stoichiometric coefficients #x, y#: are the reactant orders The … Question: Determine the reaction quotient expression for the reversible reaction below.4x10^-2 atm, pI2=4. A reaction vessel contains 0. For the reaction H2(g)+I2(g)⇌2HI(g), Kc = 55.9 g I2.016.200 M, and [HI] = 3. Question: The standard free energy of formation of gaseous hydrogen iodide is1.200 M, and [HI] = 3.5, What were the equilibrium concentration for H2, I2 and HI? N2 (g) + 3 H2 (g) ↔ 2 NH3 (g) ΔH = −92kJ/mol. HI (g) is introduced into five identical 400-cm3 glass bulbs, and the five bulbs are maintained at 623 K.6 x 10-3 L mol-1 s-1 at 700 °C.26 atm pressure of HI is admitted to the container, and it is allowed to come to equilibrium again.7. What will be the concentration of HI after t = 9.0 = ]2I[ ,M 001. Consider the following system at equilibrium at 698 K: 2HI (g) H2 (g) + I2 (g) When some HI (g) is added to the equilibrium system at constant temperature: The reaction must: fill in the blank 1 A.25 * 10^(3)# Explanation: You Step 4: Substitute Coefficients and Verify Result. calculate the concentrations of all species when equilibrium is reached. Shown below is an incomplete energy diagram for the reaction.0900 MM .100 M, [I2] = 0. What is the equilibrium constant, Kc, for the reaction at this temperature? H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3. 2HI(g) H2(g) I2(g) K for the reaction is 0.059 g H2 and 4.27 mol/L I have the answer but need to see the work. B. At the start of the reaction there are 0.200 M, and [HI] = 3. Find Kp for the reaction 2HI (g) H2 (g)+ I2 (s) at this temperature. Transcribed image text: 25.8. If the initial concentration of HI in a container is 3.200 M, and [HI] = 3. 2HI (g) H2 (g) + I2 (g) Calculate the equilibrium concentrations of reactant and products when 0.100 M, [I2] = 0. Chemistry.00-L reaction vessel at 400ºC.484 M , [I2]=0. Question: The decomposition of hydrogen iodide, 2HI (g) ----> 2H2 (g) + I2 (g), has rate constants of 9. Copy link.220 M e.75M and [I2]=2. Calculate the concentration of HI at equilibrium. What is the value of Keq for the equilibrium below? 1/2H₂ (g) + 1/2 I₂ (g) ⇌ HI (g), The value of Keq for the equilibrium H₂ (g) + I₂ (g) ⇌ 2 HI (g) is 794 at 25°C. ÐÏ à¡± á> þÿ h j Exercise 14. See Answer Question: For the reaction: 2HI (g) ↔ H2 (g) + I2 (g) Keq = 0. To form HI The equilibrium constant, Kc, for the following reaction is 1.0 minutes? 1 pts. The potential energy of the reactants is indicated on the diagram. Part A.60 mol/L, [H2] = .6 g HI.39 M HI and no product. Chemistry questions and answers. A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine:2HI (g) ↔ H2(g) + I2(g)When the system comes to equilibrium at 425 °C, PHI = 0. The equilibrium constant, Kc, for the following reaction is 1.42 mol of H2 were placed in a 1.6x10^-1 atm. About us. Unlock. What will be the concentration of HI after t = 4. Shown below is an incomplete energy diagram for the reaction. Thanks! HI decomposes to H2 and I2 by the following equation: 2HI (g) → H2 (g) + I2 (g);Kc = 1.0 M HI is placed into a closed container and the reaction is allowed to reach equilibrium at 25∘C, what is the equilibrium concentration of H2 (g)? The equilibrium constant, Kc, for the reaction H2 (g) + I2 (g) ⇄ 2HI (g) at 425°C is 54. Run in the reverse direction to restablish equilibrium. 2HI (g) H2 (g) + I2 (g) K = [H2] [I2] = 2. Kc = 56.00-L flask containing an equilibrium mixture of the three gases, there are 0. Answer to Solved Calculate Kc for the reaction 2HI(g) = H2(g) + I2(g) Science; Chemistry; Chemistry questions and answers; Calculate Kc for the reaction 2HI(g) = H2(g) + I2(g) given that the concentration of each species at equilibrium are as follows: [HI] = 0., As the reaction quotient Q increases, what is the effect on the Chemistry questions and answers.85 mol/L, [I2] = . What is the value of KcKc at this temperature? Express the equilibrium constant to three significant digits. Equilibrium concentration of H1 decreases 3. 0. Chemistry questions and answers.40-L reaction chamber.G.040. H2 (g) + I2 (g) yields (k1 on top of the arrow) 2HI (g) (one step reaction)Mechanism b. (a) Assuming ideal gas behavior, calculate the mass of H 2 present in the reaction mixture at equilibrium. Show transcribed image text. The potential energy of the reactants is indicated on the diagram.761 g H2 and 96. Chemistry questions and answers.64 moles of HI (g), 0. 0. Express your answer in moles per liters to three significant figures.3 kg of CH 4 and 55. The value of Keq for this reaction is _____. What is the equilibrium constant for the reaction H2(g)+I2(g)⇌2HI(g) at 700 K? Express your answer using two significant figures.638 0.0249 0. The standard free energy of formation of gaseous hydrogen iodide is1.0411 0.68×1010 s ([HI]t for a reaction starting under the condition in the simulation? k = 6. The reaction described by H2 (g) + I2 (g) yields 2HI (g) has an experimentally determined rate law of rate of reaction= k [H2] [I2]some proposed mechanisms for this reaction are: Mechanism a. A) 4 Fe (s) + 3 O2 (g) 2 Fe2O3 (s) B) H2 (g) + Cl2 (g) 2 HCl (g) C) 2HI (g) H2 (g) + I2 (g) D) 2 SO3 (g) 2 SO2 (g) + O2 (g) E) N2 (g) + 3 H2 (g) 2 NH3 (g), 43) Of the following equilibria, only _____ will shift to the left in H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3. Question: At 500 °C, hydrogen iodide decomposes according to 2HI(g)↽−−⇀H2(g)+I2(g) For HI(g) heated to 500 °C in a 1.033M, and 0. Step 1.50 s is found to be 0.6} \] Increasing the temperature of the reaction increases the internal energy of the system. Chemistry.2.0890 M HI, 0. H2 (g) + I2 (g) ⇋2HI (g) is 794 at 25 °C.78 atm O 0. 1)For the reaction in the previous problem, that is, 2HI (g) ↔ H2 (g) + I2 (g) Keq = 0.00 mol of HI(g) is introduced into the reaction vessel, what are 2HI(g)⇌H2(g)+I2(g) Select the correct answer below: Qc=[HI]2[H2][I2] Qc=[H2][I2][HI] Qc=[H2][I2][HI]2.215 M H 2, and 0. The equilibrium constant, Kp, for the reaction H2(g) + I2(g) ⇌ 2HI(g) at 25°C can be calculated using the standard Gibbs free energy change, ΔG°, of 2. The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) is 794 at 25 °C. Chemistry Chemistry questions and answers Determine the reaction quotient expression for the reversible reaction below. 2HI (g)?H2 (g)+I2 (g) This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.80×10-2 at 698 2HI(g) --> H2(g) + I2(g) Rate = -d[HI]/dt = k = 1." Russian media reported that two unmanned The Battle of Moscow was a military campaign that consisted of two periods of strategically significant fighting on a 600 km (370 mi) sector of the Eastern Front during World War II, between September 1941 and January 1942. If an additional 1. The system H2(g) + I2(g) ⇌ 2HI(g) is at equilibrium at a fixed temperature with a partial pressure of H2 of 0.6 x 10-3 L mol-1s-1 at 700 ºC. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. The following reaction was performed in a sealed vessel at 723 ∘C : H2 (g)+I2 (g)⇌2HI (g) Initially, only H2 and I2 were present at concentrations of [H2]=3. Chemistry Chemistry questions and answers For the reaction 2HI (g)⇌H2 (g)+I2 (g), the equilibrium constant Kc=1.25 Consider the reaction: H2 (g) +I2 (g) 2 HI (g) A reaction mixture in a 3.3 HI(g) 25. (Express your answer to four significant figures and include the appropriate units.0×10−3M and the initial concentrations of H2, and the initial concentrations of H2, and I2 are both 1. at 825 K.8×10−2 at 700 K..80×10-4 mol L-1 s-1 If the experiment has an initial HI concentration of 0. Given the partial pressures of HI, H2 and I2 at equilibrium (PHI = 0. 0.00 L container to react.414 M, and [HI] = 3. 2HI (g) → H2 (g) + I2 (g) The rate constant for this reaction is 1. Consider the reaction: 2 HI (g) ⇌ H₂ (g) + I₂ (g) Kc = 7. 0. Part A. Chemistry questions and answers. a.08 ×10 −25 at 25∘C (d) H2O(I) ⇌ H2O(g) KP = 0.5 k J/m o l r x n H 2 (g) and I 2 (g) can react to produce HI (g) , as represented above.275 M The value of Keq for the equilibrium.10x10^-5 L/mol*s / 9. What is the equilibrium constant, KcKcK_c, for the The decomposition of HI is described by the following equations: 2HI(g) -----> H2(g) + I2(g) R = k [HI]2 At 400 oC, the rate constant k has the value 8. The equilibrium concentration of I2 is 0.s-1 : 2HI (g) → H2 (g) + I2 (g) 1) Based on the units of the rate constant, is the reaction first order or second order? Explain.0% reacted at 731 K.300 mol of H2 and 0. The temperature is expressed as the absolute temperature in Kelvin. Consider the equilibrium system involving the decomposition of hydrogen iodide.T.100 M, [I2] = 0. Calculate K for 2HI (g)⇌H2 ( g)+I2 ( g) at this temperature.00 x 102 for the reaction H2 (g) + I2 (g) <-> 2HI (g) In an experiment, 1.swal etar no noitseuq yrtsimehC neewteb muirbiliuqe eht rof ,)Jk( ° G Δ ,egnahc ygrene eerf eht si tahW )g( IH2 → )g( 2I + )g( 2H 020.00 L reaction vessel that contains 20. HI decomposes to H2 and I2 by the following equation: 2HI (g) → H2 (g) + I2 (g);Kc = 1.95M[I2]=2.2.] = 0.5 L container at 758 K, the value of the equilibrium constant, Kc, is. Run in the forward direction to restablish equilibrium. What will be the concentration of HI after t = 4.9) The equilibrium constant expression for this reaction is.00 mole of I2, and 1.

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The law of mass action best fits which of the following descriptions? Find the equilibrium expression for the reversible reaction below.2 at 430 degree C. 21. B.Q.53×1010 s ([HI]t) for a reaction starting under the condition in the simulation? Given from simulation: Rate Law: k[HI]^2 k= 6. only products are Question: Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. The decomposition of hydrogen iodide follows the equation 2HI ( g) → H2 ( g) + I2 ( g). If an additional 1.27 mol/L I have the answer but need to see the work. 2HI(g) H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.00 L reaction vessel at 400ºC. H2 (g) + I2 (g) yields (k1 on top of the arrow) 2HI (g) (one step reaction)Mechanism b. 2HI(g)?H2(g)+I2(g) Here’s the best way to solve it.60 mol/L, [H2] = .The amount of I2 produced over time is measured by opening each 2HI(g)⇌H2(g)+I2(g)2HI(g)⇌H2(g)+I2(g) At equilibrium it is found that [HI]=[HI]= 3. 2HI (g) leftright arrow H2 (g) + I2 (g) What will happen to the reaction mixture at equilibrium if some H2 (g) is removed? A) The equilibrium will shift to the left.498 M I 2. Reaction Information Word Equation … H2 + I2 = HI is a Synthesis reaction where one mole of Dihydrogen [H 2] and one mole of Diiodine [I 2] combine to form two moles of Hydrogen Iodide [HI] Show Chemical … Finally, the standard molar Gibbs Free Energies at 298.072 M, what was the initial concentration of HI? H2 (g) + I2 (g) ⇌ 2HI (g) Kc=54.00623 mol of H2, 0. Show transcribed image text.75-L flask at a certain temperature initially contains 0. For the reaction H2(g) + I2(g) ⇌ 2HI(g) K= 57.00160 M-1 . products predominate b.15) K p = K ( R T) Δ n.6 × 10−3 2 H I ( g ) → H 2 ( g ) + I 2 ( g ) ; At 25 C If 1. (b) What is the percent yield of the reaction under these conditions? (not answered) Consider the following exothermic reaction below.7.70 M I₂, the what is the equilibrium concentration of HI? MULTIPLE CHOICE.38 x 10-4 mol-1 L s-1 and at 500 oC, the rate constant k has the value 7.20M. In a certain experiment the decomposition of hydrogen iodide on finely divided gold is zeroth order with respect to HI. View the full answer. Chemistry questions and answers.0275 M c.51x10^-9 L/mol*s) ( (1/ The value of Keq for the equilibrium H2 (g) + I2 (g) ⇌ 2HI (g) is 794 at 25 °C.00 mol of HI (g) is introduced into the reaction vessel In which direction will the position of the equilibrium be shifted for each of the following changes? Explain your answers.643 moles of I2 are at equilibrium in a 17. C. 1.250 M 0 We know the reaction proceeds from left to right because there is no HI present initially and the equilibrium amount of HI is 0. (Please show me the step-by-step math needed to achieve this 2 H I (g) ⇌ H 2 (g) + I 2 (g), For the above reaction the degree of dissociation ( α ) of HI (g) is related to equilibrium constant K p by the expression : View Solution The concentrations of HI and I2 will increase as the system is approaching. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Hydrogen iodide decomposes according to the equation shown below. 2H18) <--> H2(g) + 12(g) + heat Shift (Left, Right, or no shift) Change Reason Hydrogen is added lodine is removed Some argon is added Volume of container is doubled Volume of container is doubled Temperature is decreased The reaction vessel is heated Edit View Insert Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0and the rate constant k for the reaction. If an additional 1. Solution. a. Which statement is correct about this reaction mixture? View Available Hint(s) The equilibrium constant, Kc, for the reaction H2 (g) + I2 (g) ⇄ 2HI (g) at 425°C is 54. 1. For the reaction in the previous problem, that is, 2HI (g) ↔ H2 (g) + I2 (g) Keq = 0.00 L vessel where the following equilibrium was established: H2 + I2 <-----> 2HI For this reaction, Kc = 49. See Answer Balanced Chemical Equation 2 HI → H 2 + I 2 ⬇ Scroll down to see reaction info and a step-by-step answer, or balance another equation.Ea = - (8.K 137 ta 2-01×59.3 at 700 K. What is the equilibrium constant for the reaction H2 (g)+I2 (g)⇌2HI (g) at 700 K? This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.80×10-2 at 698 K. A reaction vessel contains 0.6} \] Increasing the temperature of the reaction increases the internal energy of the system.a seciohc rewsna fo puorG ?muirbiliuqe ta IH fo noitartnecnoc eht si tahW .250 M 0.886 mole of HI in a 2.50 M? [H2] = 0.0.550 mol HI was injected into a 2.0244 Question: In an experiment hydrogen iodide was found to be 24. [4] The reaction will stop.53 M0. Find [H2] at 340 ∘C . Who are the experts? Experts have been vetted by Chegg as specialists in this subject.80×10-2 at 698 2HI(g) --> H2(g) + I2(g) Rate = -d[HI]/dt = k = 1.) b) Calculate the equilibrium constant, K.Moscow was one of the primary military and political It was the latest step in an ongoing crackdown on L. Thank you.6 g HI.0156 at 400ºC. + 2 H2(g) ⇌ CH3OH (g)In an experiment, 0. We reviewed their content and use your Final answer.0=]2H[ :muirbiliuqe ta snoitartnecnoc eseht denimreted sisylana lacimehc ,lessev noitcaer L 00.148 atm of HI(g) is sealed in a flask, what is the pressure of each gas when equilibrium is established What is the standard free energy change, ΔG°, for the reaction shown below at 453°C? 2HI(g) ↔ H2(g) + I2(g) Kp = 0. The rate constant for the decomposition of hydrogen iodide (HI) at 700oC equals 0.27 mol/L. At equilibrium, the flask contains 90. What will be the concentration of HI after t = 9. Will the equilibrium concentration of HI increase, decrease, or remain See Answer.0049. 2HI(g)?H2(g)+I2(g) Determine the reaction quotient expression for the reversible reaction below. At equilibrium, the flask contains 90. Drag the appropriate items to their respective bins. Question: Assuming all gases are at the same temperature and pressure, how many milliliters of hydrogen iodide are produced from 150 mL of H2? H2 (g)+I2 (g)→2HI (g) Express your answer with the appropriate units.15) K p = K ( R T) Δ n.

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.100 mol I2 were placed in a 1. Question: What is the free energy change, ΔG°, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 311°C? Kc = 0.32 g I2.10M and [I2]=2. The equilibrium constant, Kc, for the following reaction is 1.82 × 10-1. [HI] = M [H2] = M [I2] = M. HI (g) is introduced into five identical 400-cm3 glass bulbs, and the five bulbs are maintained at 623 K. Who are the experts? Experts have been vetted by Chegg as specialists in this subject.59×10 −3 MM , [H2]=[H2]= 4.2 kJ/mol).428 moles of H2, and 0. H2 (g)+I2 (g) = 2HI (g) At this temperature, 0. H2 (g) + I2 (g) → 2HI (g) A student makes the following statements: Hydrogen always has the same oxidation number, so it has an oxidation number of +1 in both the reactant H2 and product HI.0960 atm. Science. Who are the experts? Experts are tested by Chegg as specialists in their subject area.43×10-2 at 1110 K.55M.2HI (g) -> H2 (g) + I2 (g) There are 2 Hydrogen atoms and 2 Iodine atoms on the right so the have to be 2 of each on the left as well, so there are 2 HI molecules on the left.50×10-3M at 400 K, which one of the following statements is H2(g) + I2(g) ⇌ 2HI(g) and more.95×10-2 at 731 K.75-L flask at a certain temperature initially contains 0. [3] There is no effect on the equilibrium. Chemistry.00 mol of HI(g) is introduced into the reaction vessel, what are 2HI(g)⇌H2(g)+I2(g) Select the correct answer below: Qc=[HI]2[H2][I2] Qc=[H2][I2][HI] Qc=[H2][I2][HI]2. 2HI (g) H2 (g) + I2 (g) Calculate the equilibrium concentrations of reactant and products when 0. Calculate the magnitude of Kc for the reaction. Chemistry questions and answers. Step 4: Substitute Coefficients and Verify Result. What is the rate of appearance of I2 over the same period? a. What is the activation energy of this reaction? Question: Given a reversible chemical reaction: H2(g) + I2(g) ⇌ 2HI(g) Kc = 64.00 L vessel at 698 K.4 x 10-2 M, how many minutes will it take for the concentration to be reduced to 8.15) (15. Phản ứng giải phóng nhiệt lượng 11,3 kJ khi 2 mol HI được tạo thành. The answer is . B. 0.45 M HI and no product. Tổng nhiệt phá vỡ liên kết của chất phản ứng lớn hơn nhiệt tỏa ra khi tạo thành Question: Hydrogen iodide decomposes according to the equation 2HI(g) H2(g) + I2(g), for which Kc = 0. Assume that all concentrations are equilibrium concentrations in M . See answers. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.87×10 −4 MM .

00 L reaction vessel at 400ºC

.122 at For the reaction 2HBr(g) ⇌ H2(g) + Br2(g) K = 2. If 1. What is the rate constant at 645 K? The activation energy for the decomposition of HI(g) to H_2(g) and I_2(g) is 186 kj/mol.56×10−3 M , [H2]= 4.484 M , [I2]=0. At equilibrium, _____. B.100 atm.13 M1.0 g of HI (g) is injected into a 4. Kp = K(RT)Δn (15. Study with Quizlet and memorize flashcards containing terms like Calculate Kc for the reaction 2HI(g) ⇌ H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows:[HI] = 0. H2(g) + I2(g) 2HI(g) Initial 0.0156 at 400ºC. Consider the following reaction: 2HI (g) H2 (g) + I2 (g) If 3. 0.s at 500 K Express your answer in moles per liters to On one set of axes, sketch concentration vs time curves for H2 and HI.016 Initially a container contains 0. 0. The reaction is second order and has a rate constant equal to 1.393 M. At 500 °C, hydrogen iodide decomposes according to 2 HI (g) — H2 (g) +1_ (8) For HI (g) heated to 500 °C in a 1. Please show work. For the reaction 2HI(g) H2(g) +I2(g), the degree of dissociation (a) of HI(g) is related to equilibrium constant kp by the relation? Open in App.0552 mol of HI in a volume of 735 cm3 .390 mol/L, what is the concentration of HI after 28.353 moles of HI are introduced into a 1. The reaction described by H2 (g) + I2 (g) yields 2HI (g) has an experimentally determined rate law of rate of reaction= k [H2] [I2]some proposed mechanisms for this reaction are: Mechanism a. 1)For the reaction in the previous problem, that is, 2HI (g) ↔ H2 (g) + I2 (g) Keq = 0. Use data from Appendix C to calculate the equilibrium constant, K, and Δ G ∘ at 298 K for each of the following reactions. Which statement is correct about this reaction mixture? Expert Answer.10 x 10^-5 L/mol*s at 600 K.314 J/mol*K) (ln 1. Expert-verified.5x10^-3 atm and pHI=2. a) H2 ( g )+I2 ( g )⇌2HI ( g) Calculate Δ G ∘.30 kJ/mol at 25°C.07x1010 s ( [HI]+) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures.290 at 400 K. If the initial concentrations of H2 and I2 are both 0. Balance the This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. [HI] = M [H2] = M [I2] = M.336 M hydrogen iodide.038 but I need detailed steps how to get there.15M, 0.00414 mol of I2, and 0. When the system comes to equilibrium at 400°C, what will be the total pressure inside the reaction vessel? 2HI (g) % H2 (g) + 12 (g), Kc = 0. Bin options: 1. The reaction. The equilibrium concentration of I2I2 is 0. H2 (g)+I2 (g)↽−−⇀ 2HI (g)𝐾= [HI]2 [H2] [I2]H2 (g)+I2 (g)↽−−⇀ 2HI (g)K= [HI]2 [H2] [I2] For the reaction 2HI (𝑔)↽−−⇀ H2 (𝑔)+I2 (𝑔)2HI (g)↽−−⇀ H2 (g)+I2 (g) select the equilibrium constant Hydrogen iodide can decompose into hydrogen and iodine gases.00 L vessel at 698 K.51x10^-9 L/mol*s) ( (1/ The value of Keq for the equilibrium H2 (g) + I2 (g) ⇌ 2HI (g) is 794 at 25 °C.714 mole of H2, 0. What is the reaction quotient, Q, for this system when [H2] = 0. Find step-by-step Chemistry solutions and your answer to the following textbook question: Hydrogen iodide decomposes according to the reaction $2 \mathrm { Hl } ( \mathrm { g } ) \rightleftharpoons \mathrm { H } 2 ( \mathrm { g } ) + 12 ( \mathrm { g } )$ A sealed 1. K = [HD]2 [H2][D2] (15.50 M.85 mol/L, [I2] = . Shown below is an incomplete energy diagram … For the reaction 2HI(g) H2(g) +I2(g), the degree of dissociation (a) of HI(g) is related to equilibrium constant kp by the relation? Open in App.45 M HI and no product.8. The reaction described by H2 (g) + I2 (g) yields 2HI (g) has an experimentally determined rate law of rate of reaction= k [H2] [I2]some proposed mechanisms for this reaction are: Mechanism a. What is the value of Kc at this temperature? Chemistry questions and answers. Question: Gaseous hydrogen iodide is placed in a closed container at 425∘C, where it partially decomposes to hydrogen and iodine: 2HI(g)⇌H2(g)+I2(g) At equilibrium it is found that [HI]= 3.6 × 10−3 at 25∘C.2. What is the value of KcKc at this temperature? Express the equilibrium constant to three significant digits.138 M d. Suggest Corrections. What is the mass of HI in the flask? Senior News Reporter.390 mol/L, what is the concentration of HI after 28.484 M , and [HI]=4.3 at 430 degree C.353 moles of HI are introduced into a 1. View the full answer. ÐÏ à¡± á> þÿ h j Exercise 14. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Copy link.0 at 700 K what can be said about this reaction at this temperature? A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: (2pt) 2HI(g) H2( g)+I2( g) When the system comes to equilibrium at 425∘C,PHi=0. Hydrogen iodide decomposes according to the equation 2HI (g) H2(g) + I2(g), Question: Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. Qc=[HI][H2][I2] There are 2 steps to solve this one. Suppose 0. Equilibrium concentration stays. Find Ea. at a particular temperature, K= 1. Mar 4, 2018 #K_c = 2. Express your answer using two significant The decomposition of HI (g) is represented by the equation 2HI (g) = H2 (g) + I2 (g) The following experiment was devised to determine the equilibrium constant of the reaction.10M and [I2]=2.50 M? 613. Shown below is an incomplete energy diagram for the reaction.60 M HI, 0. Thus, increasing the temperature has the effect of increasing the amount of one of the products of this reaction. (a) N2 (𝑔)+O2 (𝑔) 2NO (𝑔) T=2000°C 𝐾𝑝=4. ΔG°, for the reaction shown below at 453°C? 2HI(g) ↔ H2(g) + I2(g) Kp = 0. Solution. 0.) Convert the values of Kc to values of K p or the values of K p to values of Kc.80×10-2 at 698 K. Reaction Information Word Equation Hydrogen Iodide = Dihydrogen + Diiodine Consider the gas-phase reaction H2 (g) + I2 (g) ⇄ 2 HI (g) Suppose that a sealed flask containing H2 and I2 has been heated to 425 °C and the initial concentrations of H2 and I2 were each 0.The Soviet defensive effort frustrated Hitler's attack on Moscow, the capital and largest city of the Soviet Union.87×10 −4 MM , and [I2]=[I2]= 4. 2HI(g)⇌H2(g)+I2(g) Kc=[H2]/[I2][HI]^2.