The equilibrium constant, K, for the following reaction is 5.10×10-6 at 548 K.NH4Cl(s) NH3(g) + HCl(g)An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.396 mol NH4Cl, 2.26×10-3 M NH3 and 2.26×10-3 M HCl. If the concentration of NH3(g) is suddenly increased to 4.09×10-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished?

The objective of the question is to calculate the concentrations of the two gases.

Answered: The equilibrium constant, K, for the…

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

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The equilibrium constant, K, for the following reaction is 5.10×10^-6 at 548 K.
NH₄Cl

(s)

NH₃

(g) +

HCl

(g)

An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.396 mol NH₄Cl, 2.26×10^-3 M NH₃ and 2.26×10^-3 M HCl. If the concentration of NH₃(g) is suddenly increased to 4.09×10^-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished?

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