The equilibrium constant, Kp , for the following reaction is 1.04×10-2 at 548 K.NH4Cl(s) NH3(g) + HCl(g)If an equilibrium mixture of the three compounds in a 7.35 L container at 548 K contains 2.11 mol of NH4Cl(s) and 0.210 mol of NH3(g), the partial pressure of HCl(g) is atm.
The equilibrium constant, Kp , for the following reaction is 1.04×10-2 at 548 K.NH4Cl(s) NH3(g) + HCl(g)If an equilibrium mixture of the three compounds in a 7.35 L container at 548 K contains 2.11 mol of NH4Cl(s) and 0.210 mol of NH3(g), the partial pressure of HCl(g) is atm.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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The equilibrium constant, Kp , for the following reaction is 1.04×10-2 at 548 K.
NH4Cl(s) NH3(g) + HCl(g)
If an equilibrium mixture of the three compounds in a 7.35 L container at 548 K contains 2.11 mol of NH4Cl(s) and 0.210 mol of NH3(g), the partial pressure of HCl(g) is atm.
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