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3. Consider the following reaction: NH,HS(s) NH3(g) + H,S(g) At a certain temperature, K.= 8.5 x 10, A reaction mixture at this temperature containing solid NH.NS has [NH] = 0.166 M and [H,S] = 0.166. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached? Calculation must be shown to support your answer. More solid

3. Consider the following reaction: NH,HS(s) NH3(g) + H,S(g) At a certain temperature, K.= 8.5 x 10, A reaction mixture at this temperature containing solid NH.NS has [NH] = 0.166 M and [H,S] = 0.166. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached? Calculation must be shown to support your answer. More solid

Chemistry
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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F d6d35969-. F Mt. Sac | My... d6P35969-... d6d35969-... d. The catalyst is added Question III A. Consider the following reaction: NH,HS(s) NH3(g) At a certain temperature, K. = 8.5 x 10, A reaction mixture at this temperature containing solid NH.NS has [NH] = 0.166 M and [H,S] = 0.166. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached? Calculation must be shown to support your answer. + H,S(g) More solid 3
Transcribed Image Text:F d6d35969-. F Mt. Sac | My... d6P35969-... d6d35969-... d. The catalyst is added Question III A. Consider the following reaction: NH,HS(s) NH3(g) At a certain temperature, K. = 8.5 x 10, A reaction mixture at this temperature containing solid NH.NS has [NH] = 0.166 M and [H,S] = 0.166. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached? Calculation must be shown to support your answer. + H,S(g) More solid 3
Expert Solution
Step 1

The direction in which the reaction proceeds to reach equilibrium can be predicted by finding reaction quotient (Qc) value and comparing with equilibrium constant (Kc) value

If Qc<Kc , reaction will proceed in forward direction

If Qc>Kc , reaction will proceed in reverse direction

If Qc=Kc , reaction is at equilibrium 

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