Consider the endothermic decomposition of carbonic acid below H2CO3(ag) = CO2(8) + H2O(1) a. Where would the equilibrium shift if the amount of H2CO3 is increased? b. Where would the equilibrium shift if the amount of CO2 is increased? c. Where would the equilibrium shift if the temperature of the reaction increases? d. Where would the equilibrium shift if the volume of the system decreases at constant temperature? e. Where would the equilibrium shift if N2 gas is introduced in the system?

Consider the endothermic decomposition of carbonic acid below H2CO3(ag) = CO2(8) + H2O(1) a. Where would the equilibrium shift if the amount of H2CO3 is increased? b. Where would the equilibrium shift if the amount of CO2 is increased? c. Where would the equilibrium shift if the temperature of the reaction increases? d. Where would the equilibrium shift if the volume of the system decreases at constant temperature? e. Where would the equilibrium shift if N2 gas is introduced in the system?

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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