Solid ammonium hydrogen sulfide (NH4HS) decomposes to form ammonia gas and hydrogen sulfide gas (H2S). 2.00 moles of ammonium hydrogen sulfide were placed in a sealed 3.00 L container and the system was allowed to reach equilibrium. At equilibrium, there were 0.0328 moles of ammonia gas. Calculate the equilibrium constant for this reaction. NH4HS (s) H2S (g) NH3 (g) Initial 0.667 molL-1 0 0 Change -x +x +x Equilibrium constant 0.0328 mol 0.0328 mol
Solid ammonium hydrogen sulfide (NH4HS) decomposes to form ammonia gas and hydrogen sulfide gas (H2S). 2.00 moles of ammonium hydrogen sulfide were placed in a sealed 3.00 L container and the system was allowed to reach equilibrium. At equilibrium, there were 0.0328 moles of ammonia gas. Calculate the equilibrium constant for this reaction. NH4HS (s) H2S (g) NH3 (g) Initial 0.667 molL-1 0 0 Change -x +x +x Equilibrium constant 0.0328 mol 0.0328 mol
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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Solid ammonium hydrogen sulfide (NH4HS) decomposes to form ammonia gas and hydrogen sulfide gas (H2S).
2.00 moles of ammonium hydrogen sulfide were placed in a sealed 3.00 L container and the system was allowed to reach equilibrium. At equilibrium, there were 0.0328 moles of ammonia gas.
Calculate the equilibrium constant for this reaction.
NH4HS (s) | H2S (g) | NH3 (g) | |
Initial | 0.667 molL-1 | 0 | 0 |
Change | -x | +x | +x |
Equilibrium constant | 0.0328 mol | 0.0328 mol |
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