Consider the following homogeneous gaseous equilibrium for the synthesis of methanol:
CO(g)+2H2(g)⇌CH3OH(g)\text{CO}(\text{g}) + 2\text{H}_2(\text{g}) \rightleftharpoons \text{CH}_3\text{OH}(\text{g})CO(g)+2H2(g)⇌CH3OH(g)
Initially, 12.0 mol of carbon monoxide and 25.0 mol of hydrogen are placed in a sealed vessel. When the mixture reaches equilibrium at a certain temperature, it is found to contain 3.20 mol of methanol. Calculate the equilibrium amounts, in moles, of carbon monoxide and of hydrogen.
A different equilibrium mixture of carbon monoxide, hydrogen, and methanol is established at a temperature TTT. At equilibrium, the mixture contains 4.20 mol of carbon monoxide, 7.50 mol of hydrogen, and 2.30 mol of methanol. The total pressure of the mixture is 1200 kPa.
Calculate the value of the equilibrium constant, KpK_{\text{p}}Kp, for this reaction at temperature TTT, and state its units. Give your answer to 3 significant figures.