Question

According to LeChatelier's principle, when the reaction quotient is less than the equilibrium constant of a reaction, the reaction:

A. Must shift toward products to reach equilibrium.

B. Must shift toward reactants to reach equilibrium.

C. Results in an increase in standard enthalpy of formation of reactants.

D. Results in an increase in standard enthalpy of formation of products.

Answer 1

If the reaction quotient (Q) is less than the equilibrium constant (K), the reaction shifts toward products to increase Q and reach equilibrium.

Step-by-step explanation:

According to LeChatelier's principle, when the reaction quotient (Q) is less than the equilibrium constant (K) of a reaction, the reaction must shift toward products to reach equilibrium.

This is because the reaction needs to produce more products in order to increase the value of Q until it equals K. Therefore, if Q < K, the system responds by shifting the equilibrium position to the right, resulting in an increase in product concentrations at the expense of reactants.

According to Le Chatelier's principle, if pressure is increased, then the equilibrium shifts to the side with the fewer number of moles of gas.

This particular reaction shows a total of 4 mol of gas as reactants and 2 mol of gas as products, so the reaction shifts toward the products side.