**Equilibrium Constant and Partial Pressure Calculation**The equilibrium constant, \( K_p \), for the reaction is given as \( 1.04 \times 10^{-2} \) at a temperature of 548 K.**Chemical Reaction:**\[ \text{NH}_4\text{Cl}(s) \rightleftharpoons \text{NH}_3(g) + \text{HCl}(g) \]**Problem Statement:**In an equilibrium mixture of the three compounds within a 6.78 L container at 548 K, the following quantities are present:- 2.85 mol of \(\text{NH}_4\text{Cl}(s)\) - 0.113 mol of \(\text{NH}_3(g)\)**Question:**Calculate the partial pressure of \(\text{HCl}(g)\) in the system. **Explanation:**This problem requires the application of the equilibrium constant to determine the unknown partial pressure of HCl in a gaseous state, given the state of the reaction at equilibrium.

Answered: Image /qna-images/answer/a97abf05-4a94-4600-a7eb-85769c146dda.jpg

The equilibrium constant, Kp, for the following reaction is 1.04x10-² at 548 K. NH4Cl(s) NH3(g) + HCI(g) If an equilibrium mixture of the three compounds in a 6.78 L container at 548 K contains 2.85 mol of NH4CI(s) and 0.113 mol of NH3(9), the partial pressure of HCI(g) is atm.

The equilibrium constant, Kp, for the following reaction is 1.04x10-² at 548 K. NH4Cl(s) NH3(g) + HCI(g) If an equilibrium mixture of the three compounds in a 6.78 L container at 548 K contains 2.85 mol of NH4CI(s) and 0.113 mol of NH3(9), the partial pressure of HCI(g) is atm.

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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