6. Use Le Chatelier's principle to determine whether the equilibrium for the endothermic reaction below shifts to the left, right, or does not change under each condition listed: 4Fe) + 30 2Fe₂Ox - a. The pressure is increased b. The temperature is raised c. Some iron is added d. Some oxygen is removed

6. Use Le Chatelier's principle to determine whether the equilibrium for the endothermic reaction below shifts to the left, right, or does not change under each condition listed: 4Fe) + 30 2Fe₂Ox - a. The pressure is increased b. The temperature is raised c. Some iron is added d. Some oxygen is removed

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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The equilibrium constants at a fixed temperature for several reactions are listed below. Which equilibrium constant indicates a reaction that is favored in the forward direction? a. Keq = 1.0 × 10^5 b. Keq = 1.0 × 10^-5 c. Keq = 1.0 d. Keq = 0.0 e. none of the above choices
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?
NH3(g) + H2O(l) → NH2 + + H3O+ t The equilibrium constant is 1 x 10 -34. Is this reaction likely to take place? Why? Choose the best answer below. a. Yes, because the equilibrium constant is very small and equilibrium will lie far to the left. b. Yes, because the equilibrium constant is very small and equilibrium will lie far to the right. c. No, because the equilibrium constant is very small and equilibrium will lie far to the right. ☐ d. No, because the equilibrium constant is very small and equilibrium will lie far to the left. Click Submit to complete this assessment.
Consider the exothermic reaction: A (g) + B (s) → 2X (g) @ 25 °C a. Propose a change in VOLUME so that the equilibrium position shifts towards the REACTANTS. b. Propose a change in TEMPERATURE so that the equilibrium position shifts towards the PRODUCTS. c. Propose a change in [A] so that the equilibrium position shifts towards the PRODUCTS.
For questions 9-13. Consider the reaction 2NOCI(g) = 2NO(g) + C12(g). If this reaction is at equilibrium, what happens when the following changes occur? 9. NOCI(g) is added O shift to right shift to left no reaction O both shifts to right and left
The decomposition of PCl5 occurs by the equilibrium process PCl5(g) = PCl3(g) + Cl2(g) DH, = 92.5 kJ mol–1 If the reaction is initially at equilibrium, explain what happens when the temperature is lowered. Select one: a. The equilibrium shifts left b. The concentration of Cl2(g) will increase c. No change d. The equilibrium shifts right
Consider the following equilibrium reaction: 2 NO (g) + O2 (g) ⇋⇋ 2 NO2 (g) What is the Kc expression? Select one: a. Kc=[NO2][NO][O2]Kc=[NO2][NO][O2] b. Kc=[NO2]2[NO]2+[O2]Kc=[NO2]2[NO]2+[O2] c. Kc=[NO]2[O2][NO2]2Kc=[NO]2[O2][NO2]2 d. Kc=2∗[NO2]2∗[NO][O2]Kc=2∗[NO2]2∗[NO][O2] e. Kc=[NO2]2[NO]2[O2]
f the value of Q is greater than K for an equilibrium reaction then a. a catalyst is necessary to achieve equilibrium. b. the reaction will proceed to the right until equilibrium is established. c. the reaction will proceed to the left until equilibrium is extablished. d. the reaction will go left or right depending on the reaction stoichiometry. e. Both (a) and (d) are correct.
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.
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