The equilibrium constant, Kp, for the following reaction is 1.04x102 at 548 K. NH4CI(S) NH3(9) + HCI(g) If an equilibrium mixture of the three compounds in a 5.40 L container at 548 K contains 2.83 mol of NH4Cl(s) and 0.186 mol of NH3(g), the partial pressure of HCI(g) is atm.

The equilibrium constant, Kp, for the following reaction is 1.04x102 at 548 K. NH4CI(S) NH3(9) + HCI(g) If an equilibrium mixture of the three compounds in a 5.40 L container at 548 K contains 2.83 mol of NH4Cl(s) and 0.186 mol of NH3(g), 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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Question

The equilibrium constant, \( K_p \), for the following reaction is \( 1.04 \times 10^{-2} \) at 548 K.

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

If an equilibrium mixture of the three compounds in a 5.40 L container at 548 K contains 2.83 mol of \(\text{NH}_4\text{Cl(s)}\) and 0.186 mol of \(\text{NH}_3\text{(g)}\), the partial pressure of \(\text{HCl(g)}\) is \(\underline{\phantom{space}}\) atm.

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