At equilibrium at 1.0 L vessel contains 17.00
mol of H2, 20.00 mol of CO2, 13.00 mol of
H2O, and 6.000 mol of CO at 427◦C.
CO2(g) + H2(g) ⇀↽ CO(g) + H2O(g)
What is the value of K at this temperature
for the reaction?
What's your problem. Write the Keq expression, substitute the equilibrium numbers in the problem, and solve for Keq.
If you still can't do it explain fully what you don't understand.
To calculate the value of K at this temperature for the given reaction, you need to use the equilibrium concentrations of the reactants and products.
The balanced equation for the reaction is:
CO2(g) + H2(g) ⇌ CO(g) + H2O(g)
At equilibrium, the concentrations of CO2, H2, CO, and H2O are as follows:
[CO2] = 20.00 mol / 1.0 L = 20.00 M
[H2] = 17.00 mol / 1.0 L = 17.00 M
[CO] = 6.000 mol / 1.0 L = 6.000 M
[H2O] = 13.00 mol / 1.0 L = 13.00 M
Now, you can use the equilibrium concentrations to calculate the value of K.
K = ([CO] * [H2O]) / ([CO2] * [H2])
Substituting the given values:
K = (6.000 M * 13.00 M) / (20.00 M * 17.00 M)
Now, calculate the value of K using a calculator or by simplifying the expression further:
K = 0.16588
So, the value of K at this temperature for the given reaction is approximately 0.16588.