Chemical Equilibrium Calculation at 700°C

What is the relation between Kp and Kc for a given reaction at 700°C?

Given the data: C2H4 (g) + H2 (g) -> C2H6 (g) with Kp = 6.6 x 10^2 at 700°C.

Explanation:

To calculate Kc for the reaction at 700°C, we can use the equation Kp = Kc(RT)^Δn, where Δn is the change in the number of moles of gas.

For the given reaction C2H4 (g) + H2 (g) -> C2H6 (g) at 700°C, the equilibrium constant Kp is provided as 6.6 x 10^2. To find Kc for this reaction at the same temperature, we can use the relation between Kp and Kc along with the ideal gas constant (R) and temperature (T).

The equation relating Kp and Kc at 700°C is: Kp = Kc(RT)^Δn, where Δn represents the change in the number of moles of gas during the reaction. For this specific reaction, Δn = (1+1) - 1 = 1, as there is a net increase of 1 mole of gas in the products compared to the reactants.

By rearranging the formula Kc = Kp / (RT)^Δn and substituting the values of Kp, R, T, and Δn, we can calculate the equilibrium constant Kc for the reaction at 700°C. The correct answer in this case is B) Kc = 1/(6.6 x 10^2).

Understanding the relationship between Kp and Kc is essential in determining the equilibrium conditions of a chemical reaction at a given temperature. By applying the correct formula and considering the stoichiometry of the reaction, we can accurately calculate the equilibrium constant for different reactions.