1) Given the reaction 2 A(g) + B(g) ↔ C (g), describe the impact (forward reaction favored/reverse reaction favored/no effect) each of the following would have on the system at equilibrium. A) Increasing the partial pressure of A. B) Decreasing the pressure. C) Allowing all of gas C to escape from the container. D) Addition of a catalyst. E) Addition of inert radon gas at a constant volume. F) Will the value for K increase or decrease with the addition of C?
1) Given the reaction 2 A(g) + B(g) ↔ C (g), describe the impact (forward reaction favored/reverse reaction
favored/no effect) each of the following would have on the system at equilibrium.
A) Increasing the partial pressure of A.
B) Decreasing the pressure.
C) Allowing all of gas C to escape from the container.
D) Addition of a catalyst.
E) Addition of inert radon gas at a constant volume.
F) Will the value for K increase or decrease with the addition of C?
Introduction
Le Chatelier’s Principle states that when a system in a state of equilibrium experiences a change in one of its variables, the system will shift to counteract the change and restore equilibrium. This principle can be applied to chemical equilibrium, where a change in temperature, pressure, or concentration of a reactant or product will cause a shift in the equilibrium position in the direction that opposes the change. Le Chatelier’s Principle can also be used to explain the behavior of a system when two opposing reactions are taking place at the same time, such as a reaction between two different solutions. The shift in the equilibrium position depends on the nature of the system, the strength of the opposing reactions, and the amount of energy available to the system. In general, Le Chatelier’s Principle can be used to predict the behavior of a system when it is subjected to some type of change and to identify the conditions necessary to maintain equilibrium.
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