Chemical Equilibrium, Acids and Bases

• The concentrations of all reactants and products are equal.

• The reaction forms more reactants at this temperature than at 450°C.

• The reaction forms more products at this temperature than at 450°C.

• The concentrations of the reactants are greater than the concentration of the product.

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• [A] >> [C]

• [A] > [C]

• [A] = [C]

• [A] << [C]

Which system will respond to a decrease in pressure by increasing the equilibrium concentration of products?

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Which statement explains the effect of increasing temperature on the production of ammonia?

• The reaction will shift to the exothermic direction to yield less ammonia.

• The reaction will shift to the endothermic direction to yield less ammonia.

• The reaction will shift to the side with more moles to yield less ammonia.

• The reaction will shift to the side with fewer moles to yield less ammonia.

Which statement is not true about systems at equilibrium?

• Equilibrium can be reached from either direction.

• No macroscopic changes in the reaction mixture can be observed.

• Products of the reaction are produced and destroyed at the same rate.

• The concentrations of reactants and products stay equal to each other.

Which of the changes below will increase the equilibrium yield of ammonia?

• introducing a catalyst

• decreasing the pressure from 200 atm to 100 atm

• increasing the temperature from 100°C to 200°C

• decreasing the temperature from 200°C to 100°C

Which equation must be for a strong acid?

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Which equation must be for a strong base?

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Which equation must be for a weak base?

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