21. At 25°C, the following reactions have the equilibrium constants notetheir equations:2 CO (g) + O₂ (g)2 H₂(g) + O₂ (g)28060Use these data to calculate K for the reaction:H₂O(g) + CO (g)--CO₂ (g) + H₂ (g)A) 3.91010B) 5.6 10C) 1.9 105D) 3.5 10³E) 2.1 1010×2 CO₂ (g)2 H₂O (g)××K-3.3 x 10°K-9.1 × 1080

Answered: Image /qna-images/answer/74f47adb-8732-47d2-93d6-1f6b1992db70.jpg

21. At 25°C, the following reactions have the equilibrium constants note their equations: 2 CO(g) + O₂ (g) 2 H₂(g) + O₂ (g) A) 3.9 B) 5.6 10 C) 1.9 105 Use these data to calculate K for the reaction: H₂O(g) + CO (g) CO₂ (g) + H2 (g) × × 1010 D) 3.5 10³ E) 2.1 1010 - 2 CO₂ (g) 2 H₂O (g) K-3.3 10P K-9.1×1080

21. At 25°C, the following reactions have the equilibrium constants note their equations: 2 CO(g) + O₂ (g) 2 H₂(g) + O₂ (g) A) 3.9 B) 5.6 10 C) 1.9 105 Use these data to calculate K for the reaction: H₂O(g) + CO (g) CO₂ (g) + H2 (g) × × 1010 D) 3.5 10³ E) 2.1 1010 - 2 CO₂ (g) 2 H₂O (g) K-3.3 10P K-9.1×1080

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the following reactions and their respective equilibrium constants: NO(g) + ½Br₂(g) = NOBr(g); K = 5.3 2NO(g) = N₂(g) + O₂(g); K = 2.1 × 10³⁰ Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction: N₂(g) + O2(g) + Br₂(g) = 2NOBr(g) Express your answer using two significant figures.
Consider the following fictional reaction: 2AB(aq) = 2A(aq) + B2(aq) K = 9.8 x 101 %3D If you start out with a 5.0 M solution of AB, A, and B2, what is the concentration of each species when the reaction reaches equilibrium. when solving this problem (more specifically, you are not allowed to put the algebra equation in your calculator to solve for x)
Consider the following general reaction:2A(g) + 2B(g) ⇌ 3C(g) The reaction was measured to have an equilibrium reaction constant (K) of 0.0100 at 100 K. If the reaction has a standard enthalpy change (ΔHrxn) of 500.3 J/mol, what should the equilibrium reaction constant be when the temperature is 800 K? (Please provide your answer to 3 significant figures.)
At a certain temperature, the equilibrium constant K for the following reaction is ×2.0510−7 : Br2g + OCl2g BrOCl g+BrClg Use this information to answer the following question. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K= 3Br2 (g) +3OCl2 (g) 3BrOCl (g) +3BrCl (g
Consider this reaction equation: A2B(g)= 2 A(g) + B(g) If you start with 1.2 M A2B, and if at equilibrium, 50% of it has decomposed, what are the equilibrium concentrations of A and B? What is the value of the equilibrium constant?
Give detailed solution
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 N,(g) + 3 H,(g) 2 NH3(g) K = 1. × 10 He fills a reaction vessel at this temperature with 10. atm of nitrogen gas and 3.9 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes tools available to you within ALEKS? no ? If you said yes, then enter the equilibrium pressure of NH, at right. atm Round your answer to 1 significant digit.
Kc=?
Consider the following reactions: CO (g) + 2 H2S (g) D CS2 (g) + H2O (g) + H2 (g) K1 = 1.3 x 105 ½ CH4 (g) + H2S (g) D ½ CS2 (g) + 2 H2 (g) K2 = 180 1. Find the equilibrium constant for: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) 2. What molecules in the steps are reaction intermediates? 3. If 0.500 atm of CO, H2, CH4, and H2O are initially placed in the same container, then given your answer in part a., determine which direction the reaction will shift in order to establish equilibrium.
Compare the following two reactions ("A" and "B"), with two different equilibrium constants, K: (A) Cl2 (g) + H2 (g) = 2HCI (g) K = 0.29 (B) I2 (g) + H2 (g) = 2HI (g) K = 1.6 x 1033 %3D Which of the following statements is correct? O Reaction "A" will proceed faster because the equilibrium constant, K, is larger O Reaction "B" will proceed faster because the equilibrium constant, K, is larger O Reaction "A" favors the production of products. O Reaction "B" favors the production of products. O None of these statements are correct.
Write the equilibrium constant expression, K, for the following reaction: (If either the numerator or denominator is blank, please enter 1.) CO(g) + Cl2 (g) 2 COCI2 (g) K=
Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 2 NH3(g) = N₂(g) + 3 H₂(g) At equilibrium, [NH3] = 0.0235 M, [N₂] = 0.119 M, and [H₂] = 0.366 M. Calculate K for the reaction at this temperature. Ke