Question

if 8.0 mol pcl5 were placed in a 4.0 l vessel and allowed to come to equilibrium, what is the equilibrium constant (kc) if equilibrium was established at 300 k leaving 2.0 mol pcl5 in the mixture?

Answer 1

To calculate the equilibrium constant (Kc) for the given reaction, use the balanced chemical equation and the concentrations of the reactants and products at equilibrium. Given that the equilibrium constant (Kp) is 4.0 × 10³¹ at 47°C, use the equation Kp = Kc(RT)Δn to calculate Kc, where R is the gas constant, T is the temperature in Kelvin, and Δn is the change in moles of gas from the reactant side to the product side.

Step-by-step explanation:

To calculate the equilibrium constant (Kc) for the given reaction, we need to use the balanced chemical equation and the concentrations of the reactants and products at equilibrium.

The balanced chemical equation for the reaction is:

H₂(g) + Cl₂(g) → 2HCl(g)

Given that the equilibrium constant (Kp) is 4.0 × 10³¹ at 47°C, we can use this value to calculate Kc using the equation Kp = Kc(RT)Δn, where R is the gas constant (0.0821 L·atm/mol·K), T is the temperature in Kelvin (300 K), and Δn is the change in moles of gas from the reactant side to the product side (2 − 1 = 1).

Substituting the values into the equation, we get:

Kp = Kc(0.0821 L·atm/mol·K)(300 K)1

4.0 × 10³¹ = Kc(0.0821 L·atm/mol·K)(300 K)

Solving for Kc, we find:

Kc ≈ 1.37 × 10³⁰