41. Given this reaction at equilibrium: 2C0(g) + 02(g) = 2C02(g). Which statement regarding the reaction is always true? * a. the rates of the forward and reverse reactions are equal O b. the reaction occurs in an open system O c. the masses of the reactants and the products are equal O d. the concentrations of the reactants and the products are equal 42. Which factors must be equal in a reversible chemical reaction at

41. Given this reaction at equilibrium: 2C0(g) + 02(g) = 2C02(g). Which statement regarding the reaction is always true? * a. the rates of the forward and reverse reactions are equal O b. the reaction occurs in an open system O c. the masses of the reactants and the products are equal O d. the concentrations of the reactants and the products are equal 42. Which factors must be equal in a reversible chemical reaction at

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...

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Consider the equilibrium reaction and its equilibrium constant expression. [ICI]? 1(g) + Cl,(g) 2 2ICI(g) K = L] C] For the reaction 2ICI(g) = 1(g) + Cl,(g) select the equilibrium constant expression. K' О к [ICI]4 2|ICÍ] [L] [CL] L][Cl] [ICI]? [ICi]* K': K' = [Ici]? K' %3D L][CL]
O O Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 0.0074: N,(g) + 0,(g) = 2NO(g) Use this information to complete the following table. Suppose a 22. L reaction vessel is filled with 0.89 mol of N, and 0.89 mol of O2. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little N2 and 02. There will be very little NO. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] 2 NO(g) N2(9)+O2(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K =] 2N2(9)+202(g) 4 NO(g) 1. Explanation Check 02021 McGraw-Hill Education All Rights Reserved Terms of U
2C02 2 2C0+0 Consider the reaction above. If pressure was increase on this equilibrium, how would that affect the amounts of reactants? O They would decrease O They would remain the same O They would increase
5. The equilibrium constant expression of a gas reaction is [CS2] [H2]* _ [CH4] [H2S]? K. Write the balanced chemical equation corresponding to this expression
Consider the equilibrium reaction shown below: 3 NO2 (g) + H2O (l) ⇋⇋ 2 HNO3 (aq) + NO (g) If the total pressure on the system is increased (by compressing the volume), how will the concentration of the NO (g) be affected? Select one: a. The concentration of NO will increase. b. The concentration of NO will decrease. c. There will be no change in the concentration of NO.
5. Consider the reaction A+B=C+ D. A friend asks the fol- lowing: "I know we have been told that if a mixture of A, B, C, and D is in equilibrium and more A is added, more C and D will form. But how can more C and D form if we do not add more B?" What do you tell your friend? Consider the following statements: "Consider the reaction