In the gas phase, formic acid forms a dimer, $2 \text{HCOOH(g)} \rightleftharpoons (\text{HCOOH})_2\text{(g)}$. For this reaction, $\Delta H^\circ = -60.1 \ \text{kJ/mol}$ and $\Delta G^\circ = -13.9 \ \text{kJ/mol}$ at 25°C. Find the equilibrium constant ($K_p$) for this reaction at 75°C.

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In the gas phase, formic acid forms a dimer, 2HCOOH(g) (HCOOH)2(g). For this reaction, ΔΗ -60.1 kJ/mol and AG = -13.9 kJ/mol at 25°C. Find the equilibrium constant (Kp) for this reaction at 75 °C. =

In the gas phase, formic acid forms a dimer, 2HCOOH(g) (HCOOH)2(g). For this reaction, ΔΗ -60.1 kJ/mol and AG = -13.9 kJ/mol at 25°C. Find the equilibrium constant (Kp) for this reaction at 75 °C. =

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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Question

In the gas phase, formic acid forms a dimer, $2 \text{HCOOH(g)} \rightleftharpoons (\text{HCOOH})_2\text{(g)}$. For this reaction, $\Delta H^\circ = -60.1 \ \text{kJ/mol}$ and $\Delta G^\circ = -13.9 \ \text{kJ/mol}$ at 25°C. Find the equilibrium constant ($K_p$) for this reaction at 75°C.

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