g Enabled: Module 2 Examination i Saved Which of these situations will result if some CH4(g) is removed from the reaction CO(g) + 3H2(g) S CH4(g) + H2O(g) at equilibrium? Multiple Choice 38 No change will occur. More CO will be produced. More CH4 and H20 will be produced. H20 will be consumed. Kp will decrease.

g Enabled: Module 2 Examination i Saved Which of these situations will result if some CH4(g) is removed from the reaction CO(g) + 3H2(g) S CH4(g) + H2O(g) at equilibrium? Multiple Choice 38 No change will occur. More CO will be produced. More CH4 and H20 will be produced. H20 will be consumed. Kp will decrease.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 3RQ

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Kp for the following reaction is 0.16 at 25 C: 2 NOBr(g) 2 NO(g) + Br2(g) The enthalpy change for the reaction at standard conditions is + 16.3 kJ/mol-rxn. Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) adding more Br2(g) (b) removing some NOBr(g) (c) decreasing the temperature (d) increasing the container volume
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant expression for the reaction. Call the equilibrium constant K1. (b) Write an equilibrium constant expression for the formation of one mole of B(g) and call the equilibrium constant K2. (c) Relate K1 and K2.
Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?
Explain why an equilibrium between Br2(l) and Br2(g) would not be established if the container were not a closed vessel shown in Figure 13.5.
Consider the reactionA(g)+B(g)C(g)+D(g). A friend asks the following: I know we have been told that if a mixture of A, B, C, and D is at equilibrium and more of 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 relationships: G = 1, H = TS, Q = 1. G = G, K = 1 Which of these relationships is(are) always true for a reaction at equilibrium?
Consider the reaction: A(g)+2B(g)+C(s)2D(g)At 25C, only A, B, and C are present. The partial pressures of A, B, and D are given as PA, PB, and PD. Equilibrium is established 18 minutes after the reaction starts. Use terms is less than (LT), is greater than (GT), is equal to (EQ), or insufficient information (X) to answer the following questions. (a) PD at 5 min PA. (b) PA at 21 min PA at 27 min. (c) PB at 7 min PB at 13 min.(d) After 20 min, more B is added. When equilibrium is reestablished, K before the addition K after the addition. (e) After 20 min, the temperature is increased to 35C. PA before the temperature increase PA after the temperature increase after equilibrium is reestablished.
The equilibrium constant for a certain reaction decreases from 8.84 to 3.25 102 when the temperature increases from 25C to 75C. Estimate the temperature where K = 1.00 for this reaction. Estimate the value of S for this reaction. (Hint: Manipulate the equation in Exercise 79.)
5.22. True or false: If for a gas-phase reaction, then all equilibrium partial pressures of reactants and products must equal . Explain your choice.
For a typical equilibrium problem, the value of K and the initial reaction conditions are given for a specific reaction, and you are asked to calculate the equilibrium concentrations. Many of these calculations involve solving a quadratic or cubic equation. What can you do to avoid solving a quadratic or cubic equation and still come up with reasonable equilibrium concentrations?
Consider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?