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Nzp+ 3Hug) NH3(g)+ energy Imagine a cylinder containing nitrogen gas (N2), hydrogen gas (H2), and ammonia gas (NH3). The chemicals in the cylinder are in a state of chemical equilibrium according to the above equation. Why would compressing the system with a piston cause the amount of ammonia to increase and the amounts of nitrogen and hydrogen L.O.6 gas to decrease? before after A shift of the equilibrium to the right would increase the number of molecules. Shifting the equilibrium to the right will cause a release of energy, B- heating the system. Compressing a gas reduces its pressure because it reduces the amount of collisions. Reducing the number of molecules helps reduce the pressure of the C- D- system.

Nzp+ 3Hug) NH3(g)+ energy Imagine a cylinder containing nitrogen gas (N2), hydrogen gas (H2), and ammonia gas (NH3). The chemicals in the cylinder are in a state of chemical equilibrium according to the above equation. Why would compressing the system with a piston cause the amount of ammonia to increase and the amounts of nitrogen and hydrogen L.O.6 gas to decrease? before after A shift of the equilibrium to the right would increase the number of molecules. Shifting the equilibrium to the right will cause a release of energy, B- heating the system. Compressing a gas reduces its pressure because it reduces the amount of collisions. Reducing the number of molecules helps reduce the pressure of the C- D- system.

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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Nug+ 3H2g =NH3)+ energy Imagine a cylinder containing nitrogen gas (N2), hydrogen gas (H2), and ammonia gas (NH3). The chemicals in the cylinder are in a state of chemical equilibrium according to the above equation. Why would compressing the system with a piston cause the amount of ammonia to increase and the amounts of nitrogen and hydrogen L.0.6 gas to decrease? before after A shift of the equilibrium to the right would increase the number of molecules. Shifting the equilibrium to the right will cause a release of energy, heating the system. Compressing a gas reduces its pressure because it reduces the amount of collisions. Reducing the number of molecules helps reduce the pressure of the B- C- D- L0.6 system.
Transcribed Image Text:Nug+ 3H2g =NH3)+ energy Imagine a cylinder containing nitrogen gas (N2), hydrogen gas (H2), and ammonia gas (NH3). The chemicals in the cylinder are in a state of chemical equilibrium according to the above equation. Why would compressing the system with a piston cause the amount of ammonia to increase and the amounts of nitrogen and hydrogen L.0.6 gas to decrease? before after A shift of the equilibrium to the right would increase the number of molecules. Shifting the equilibrium to the right will cause a release of energy, heating the system. Compressing a gas reduces its pressure because it reduces the amount of collisions. Reducing the number of molecules helps reduce the pressure of the B- C- D- L0.6 system.
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