The following acid-base reaction occurs spontaneously in the gas phase at 25.0°C:\[ \text{NH}_3(g) + \text{HCl}(g) \rightleftharpoons \text{NH}_4\text{Cl}(s) \]Calculate the equilibrium constant for this reaction at 275.65 K.### Table of Standard Gibbs Free Energies of Formation| Substance | \(\Delta G_f^\circ\) (kJ/mol) ||-----------|------------------------------|| \(\text{NH}_3 (g)\) | -17 || \(\text{HCl} (g)\) | -95 || \(\text{NH}_4\text{Cl} (s)\) | -203 |This table provides the standard Gibbs free energies of formation (\(\Delta G_f^\circ\)) for each substance involved in the reaction.

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The following acid-base reaction occurs spontaneously in the gas phase at 25.0°C: NH3(g) + HCI(g) = NHẠCI(s) Calculate the equilibrium constant for this reaction at 275.65 K. Substance AG? (kJ/mol) NH3 (g) -17 HCI (g) -95 NHẠCI (s) -203

The following acid-base reaction occurs spontaneously in the gas phase at 25.0°C: NH3(g) + HCI(g) = NHẠCI(s) Calculate the equilibrium constant for this reaction at 275.65 K. Substance AG? (kJ/mol) NH3 (g) -17 HCI (g) -95 NHẠCI (s) -203

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

The following acid-base reaction occurs spontaneously in the gas phase at 25.0°C:

\[ \text{NH}_3(g) + \text{HCl}(g) \rightleftharpoons \text{NH}_4\text{Cl}(s) \]

Calculate the equilibrium constant for this reaction at 275.65 K.

### Table of Standard Gibbs Free Energies of Formation

| Substance | \(\Delta G_f^\circ\) (kJ/mol) |
|-----------|------------------------------|
| \(\text{NH}_3 (g)\) | -17 |
| \(\text{HCl} (g)\) | -95 |
| \(\text{NH}_4\text{Cl} (s)\) | -203 |

This table provides the standard Gibbs free energies of formation (\(\Delta G_f^\circ\)) for each substance involved in the reaction.

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