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4. The value of Kp for the reaction below is 1.6 at 308 K. NH,HS(s) = NH3(g) + H2S(g) Initially, 0.50 mol of each of NH4HS, NH3, and H2S is added to a 2.0-L container. VEB How many moles of NH3 are present at a. 0.10 mol NH3 equilibrium? b. 0.20 mol NH3 c. 1.3 mol NH3 d. 2.6 mol NH3 e. 5.1 mol NH3 BIZED FO

4. The value of Kp for the reaction below is 1.6 at 308 K. NH,HS(s) = NH3(g) + H2S(g) Initially, 0.50 mol of each of NH4HS, NH3, and H2S is added to a 2.0-L container. VEB How many moles of NH3 are present at a. 0.10 mol NH3 equilibrium? b. 0.20 mol NH3 c. 1.3 mol NH3 d. 2.6 mol NH3 e. 5.1 mol NH3 BIZED FO

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 3PS: Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A...
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I'm told that the answer is A, but I can't seem to get it as a solid answer. What am I missing when solving this? I know to ignore the solid in the calculations, as well as that I need to calculate it using Kc and not Kp.

4. The value of Kp for the reaction below is 1.6 at 308 K. NHẠHS(s) = NH3(g) + H2S(g) Initially, 0.50 mol of each of NH4HS, NH3, and H2S is added to a 2.0-L container. WEB How many moles of NH3 are present at equilibrium? a. 0.10 mol NH3 b. 0.20 mol NH3 c. 1.3 mol NH3 d. 2.6 mol NH3 e. 5.1 mol NH3 IZED FOR
Transcribed Image Text:4. The value of Kp for the reaction below is 1.6 at 308 K. NHẠHS(s) = NH3(g) + H2S(g) Initially, 0.50 mol of each of NH4HS, NH3, and H2S is added to a 2.0-L container. WEB How many moles of NH3 are present at equilibrium? a. 0.10 mol NH3 b. 0.20 mol NH3 c. 1.3 mol NH3 d. 2.6 mol NH3 e. 5.1 mol NH3 IZED FOR
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