18. The oxidation of NO to NO,, 2 NO(g) + 0,(g) 2 NO,(g) is exothermic. Predict the effect of each of these changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each change is made in a constant-volume system. a) Adding more O, b) Adding more NO, ) Lowering the temperature

18. The oxidation of NO to NO,, 2 NO(g) + 0,(g) 2 NO,(g) is exothermic. Predict the effect of each of these changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each change is made in a constant-volume system. a) Adding more O, b) Adding more NO, ) Lowering the temperature

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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Suppose the following exothermic reaction UO2(s)+4HF(g) UFA(g) + 2H20(g) has already reached equilibrium. Predict the effect that each of the following changes will have on the equilibrium position. State whether the equilibrium will shift to the reactants, will shift to the products, or will not be affected. Explain your answer using Le Chatelier's Principle. a. The system was cooled. b. The reaction vessel was quadrupled. C. Uranium (IV) oxide was added to the reaction. d. The partial pressure of Uranium (IV) fluoride was decreased.
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A student ran the following reaction in the laboratory at 303 K:2NO(g) + Br2(g) 2NOBr(g)When she introduced NO(g) and Br2(g) into a 1.00 L evacuated container, so that the initial partial pressure of NO was 1.15 atm and the initial partial pressure of Br2 was 0.408 atm, she found that the equilibrium partial pressure of Br2 was 0.138 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp =
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 100. L tank with 9.9 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.50 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significan digits. K = 0
Consider the following equilibrium: CO(g) + NO2(g) ↔ CO2(g) + NO(g) At a specific temperature the equilibrium concentrations where determined to be: [CO] = 0.0033M [NO2] = 0.021M [CO2] = 0.59M [NO] = 0.59M a- Calculate the value of the equilibrium constant b- Describe the position of the equilibrium
7. Suppose for a synthesis of hydrogen fluoride from hydrogen and fluorine, 3.000 moles of H2 and 6.000 moles of F2 are mixed in a 3.000-L flask. Assume that the equilibrium constant for the synthesis reaction at this temperature is 1.15x102. H2 (g) + F2 (g) ↔ 2HF (g) What is the molar concentration of HF at equilibrium? What is the molar concentration of F2 at equilibrium? At a Kc of 4.15x103, predict the direction of the reaction if the starting concentrations are [H2]=2.30 M, [F2]= 1.25x10-3 M, and [HF]= 4.37 M