The equilibrium constant for the reaction at the given temperature is approximately 2.0, derived from the concentrations of the substances at equilibrium.
Certainly! Let's denote the change in moles of CO2 as x at equilibrium. The initial concentrations are given as:
[H2O]0 = 1.113 × 10^(-2) mol
[CO]0 = 1.490 × 10^(-2) mol
[H2]0 = 0 mol
[CO2]0 = 0 mol
At equilibrium, the concentrations become:
[H2O]eq = [H2O]0 - x
[CO]eq = [CO]0 - x
[H2]eq = [H2]0 + x
[CO2]eq = [CO2]0 + x
Given that [CO2]eq = 8.326 × 10^(-3) mol, we can express x in terms of this value:
x = [CO2]eq - [CO2]0
x = 8.326 × 10^(-3) - 0
x = 8.326 × 10^(-3) mol
Now, substitute the values into the equilibrium expression for the chemical reaction:
Kc = [H2]eq * [CO2]eq / [H2O]eq * [CO]eq
Kc = (0 + 8.326 × 10^(-3)) * (8.326 × 10^(-3)) / (1.113 × 10^(-2) - 8.326 × 10^(-3)) * (1.490 × 10^(-2) - 8.326 × 10^(-3))
After performing the calculations using a calculator it is found that
Kc ≈ 2.