At equilibrium at 1.0 L vessel contains 22.00 mol of H2, 20.00 mol of CO2, 13.00 mol of H2O, and 5.700 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?
To find the value of K at a given temperature for a reaction, you need to use the equilibrium concentrations of the reactants and products.
In this case, the given equilibrium concentrations are:
[H2] = 22.00 mol
[CO2] = 20.00 mol
[H2O] = 13.00 mol
[CO] = 5.700 mol
The balanced equation for the reaction is:
CO2(g) + H2(g) ⇀↽ CO(g) + H2O(g)
The expression for the equilibrium constant (K) can be written as:
K = ([CO] * [H2O]) / ([CO2] * [H2])
Now, substitute the given concentrations into the expression for K:
K = (5.700 mol * 13.00 mol) / (20.00 mol * 22.00 mol)
Calculating this will give you the value of K at the given temperature.