The equilibrium constant, K, for the following reaction is 5.10×10-6 at 548 K.NH,Cl(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 0.326 mol NH,CI, 2.26×10-3 M NH3 and2.26x10-3 M HCI. If the concentration of NH3(g) is suddenly increased to 3.52x10-3 M, what will be the concentrations of the two gasesonce equilibrium has been reestablished?[NH3] :M[HCI]

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The equilibrium constant, K, for the following reaction is 5.10×106 at 548 K. NH,CI(s)=NH3(g) + HC(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.326 mol NH,CI, 2.26×10-3 M NH3 and 2.26×10-3 M HCI. If the concentration of NH3(g) is suddenly increased to 3.52x10-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] =| M [HCI] M

The equilibrium constant, K, for the following reaction is 5.10×106 at 548 K. NH,CI(s)=NH3(g) + HC(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.326 mol NH,CI, 2.26×10-3 M NH3 and 2.26×10-3 M HCI. If the concentration of NH3(g) is suddenly increased to 3.52x10-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] =| M [HCI] M

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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