What is Le Châtelier’s principle? Consider the reaction 2NOCl(g) 34 2NO(g) 1 Cl2(g). If this reaction is at equilibrium, what happens when the following changes occur? a. NOCl(g) is added. b. NO(g) is added. c. NOCl(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume?
What is Le Châtelier’s principle? Consider the reaction 2NOCl(g) 34 2NO(g) 1 Cl2(g). If this reaction is at equilibrium, what happens when the following changes occur? a. NOCl(g) is added. b. NO(g) is added. c. NOCl(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
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