Question

At 200 ˚C, the equilibrium constant (Kc) for the reaction below is 2.40 x 10³:

2 NO (g) ⇌ N2 (g) + O₂ (g).

Which of the following is True at equilibrium?

a) There are more reactants than products.
b) There are more products than reactants.
c) The value of Kp is less than the value of Kc.
d) The initial concentrations of reactants must have been greater than the concentrations of reactants.

Answer 1

At 200 °C, with a Kc of 2.40 x 10³ for the reaction 2 NO (g) ⇌ N2 (g) + O2 (g), there are more products than reactants at equilibrium.

Step-by-step explanation:

At 200 °C, the equilibrium constant (Kc) for the reaction 2 NO (g) ⇌ N2 (g) + O2 (g) is 2.40 x 10³. Given that the Kc is a measure of the ratio of product concentrations to reactant concentrations at equilibrium, a high Kc value, such as 2.40 x 10³, indicates that the reaction heavily favors the formation of products. Therefore, the correct statement at equilibrium for this reaction is that there are more products than reactants.

• a) There are more reactants than products - False.
• b) There are more products than reactants - True.
• c) The value of Kp is less than the value of Kc - This can not be determined without further information.
• d) The initial concentrations of reactants must have been greater than the concentrations of reactants - This is not necessarily true, as the equilibrium favors products regardless of the initial concentrations.