For the reaction CO(g) + 2 H2(g) CH3OH(g) at 700. K, equilibrium concentrations are [H2] = 0.072 M, [CO] = 0.020 M, and [CH3OH] = 0.030 M.
Calculate K.
What would K be?
Kc = [CO][H₂]²/[CH₃OH] ... substitute given data and solve for Kc.
oops. I have corrected the post by Doc.
For the reaction CO(g) + 2 H2(g) ==> CH3OH(g)
Kc =[CH₃OH]/[CO][H₂]²
To calculate the equilibrium constant (K) for a reaction, you need to use the equilibrium concentrations of the reactants and products. In this case, the given equilibrium concentrations are [H2] = 0.072 M, [CO] = 0.020 M, and [CH3OH] = 0.030 M.
The balanced equation for the reaction is:
CO(g) + 2 H2(g) CH3OH(g)
K is calculated using the following expression:
K = [CH3OH] / ([CO] * [H2]^2)
Now, substitute the given equilibrium concentrations into the equation:
K = (0.030 M) / ((0.020 M) * (0.072 M)^2)
To calculate the final value of K, simply solve this equation.