Question

. Consider the reaction.

CaCO₃ (s) ---> Cao (s) + CO₂ (g)

An equilibrium mixture of this reaction at a certain temperature has (CO₂) = 0.548 M. What is the value of the equilibrium constant at this temperature? Is the reverse or forward reaction favored?

Answer 1

An equilibrium mixture allows prediction of the favored reaction (forward or reverse) based on the reaction quotient compared to the equilibrium constant. However, with the given information, it is not possible to determine the equilibrium constant or the favored reaction.

Step-by-step explanation:

An equilibrium mixture can be used to predict whether the forward or reverse reaction will be favored. In this case, the reaction is CO(g) + H₂O(g) = CO₂(g) + H₂(g) and the equilibrium constant (Kc) is 0.640 at a temperature of 800 °C. To determine if the reverse or forward reaction is favored, the reaction quotient (Qc) is compared to Kc.

If Qc < Kc, the reactants' concentrations are initially lower than the equilibrium concentrations, and thus, the forward reaction is favored. If Qc > Kc, the reactants' concentrations are initially higher than the equilibrium concentrations, and thus, the reverse reaction is favored.

In the given question, the equilibrium mixture has a concentration of CO₂ of 0.548 M. However, the concentration of other reactants and products is not mentioned. Without this information, we cannot determine the value of the equilibrium constant or whether the reverse or forward reaction is favored.