Consider the following equilibrium system that has an equilibrium constant, Keq, of 3.00: SO 16) + NO219) SO3(g) + NO(g) a) The initial concentrations are as follows: [SO2(e)] = 2.75M, [NO2(9)] = 0.25M, [SO3{9)] = 2.25M, [NO 9] = 1.25M Which direction will the system shift to reach equilibrium. b) Calculate the concentration of each species at equilibrium. c) If 0.85 moles of NO, gas was injected into 1.00 litre of this equilibrium system, calculate the concentrations of each gas when the second equilibrium has been reached.

Consider the following equilibrium system that has an equilibrium constant, Keq, of 3.00: SO 16) + NO219) SO3(g) + NO(g) a) The initial concentrations are as follows: [SO2(e)] = 2.75M, [NO2(9)] = 0.25M, [SO3{9)] = 2.25M, [NO 9] = 1.25M Which direction will the system shift to reach equilibrium. b) Calculate the concentration of each species at equilibrium. c) If 0.85 moles of NO, gas was injected into 1.00 litre of this equilibrium system, calculate the concentrations of each gas when the second equilibrium has been reached.

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 34QAP

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