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The reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) has ΔH° = -12.65 kJ mol-1 and ΔS° = -192.5 J mol-1 K-1. Calculate the equilibrium constant when the temperature is 50.0 °C. (R = 8.3145 J mol-1 K-1) Multiply your answer by 109 before entering it. (Hint: remember that when calculating ΔG°, all values must be for standard state.)

The reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) has ΔH° = -12.65 kJ mol-1 and ΔS° = -192.5 J mol-1 K-1. Calculate the equilibrium constant when the temperature is 50.0 °C. (R = 8.3145 J mol-1 K-1) Multiply your answer by 109 before entering it. (Hint: remember that when calculating ΔG°, all values must be for standard state.)

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 15P
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The reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) has ΔH° = -12.65 kJ mol-1 and ΔS° = -192.5 J mol-1 K-1. Calculate the equilibrium constant when the temperature is 50.0 °C. (R = 8.3145 J mol-1 K-1)  Multiply your answer by 109 before entering it. (Hint: remember that when calculating ΔG°, all values must be for standard state.)

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