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Consider the reaction N2 (g) + O2 (g) ? 2 NO (g) ?H = +43 kcal/mol...

Consider the reaction N2 (g) + O2 (g) ? 2 NO (g) ?H = +43 kcal/mol

Which of the following statements is true?
a) Increasing the temperature will favor the forward reaction, and the concentration of NO (g) will be higher at equilibrium.
b) Increasing the concentration of NO (g) will favor the forward reaction, and the concentrations of both N2 and O2 will be lower at equilibrium.
c) Adding a catalyst will favor the forward reaction, and the concentration of NO (g) will be higher at equilibrium.
d) Decreasing the pressure will increase the rate at which equilibrium is reached, but will have no effect on the final concentrations at equilibrium.

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Answer #1

Positive value of delta H indicates that it is endothermic reaction.

a) Increasing the temperature will favor the forward reaction, and the concentration of NO (g) will be higher at equilibrium. This is in accordance with Le Chateliers principle. Hence, the statement a) is correct.
b) Increasing the concentration of NO (g) will favor the reverse reaction, and the concentrations of both N2 and O2 will be higher at equilibrium. Hence, the statement b) is incorrect.
c) Adding a catalyst will favor the forward reaction and the reverse reaction to equal extent, and the concentration of NO (g) will be unaffected. Hence, the statement c) is incorrect.
d) Decreasing the pressure will decrease the rate at which equilibrium is reached, but will have no effect on the final concentrations at equilibrium. Hence, the statement d) is incorrect.

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