Consider the following equilibrium reaction for the industrial 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, 8.50 mol8.50 \text{ mol}8.50 mol of carbon monoxide and 17.20 mol17.20 \text{ mol}17.20 mol of hydrogen are placed in a sealed vessel. When the mixture reaches equilibrium at a certain temperature, it is found to contain 3.40 mol3.40 \text{ mol}3.40 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 1.25 mol1.25 \text{ mol}1.25 mol of carbon monoxide, 2.45 mol2.45 \text{ mol}2.45 mol of hydrogen, and 3.80 mol3.80 \text{ mol}3.80 mol of methanol. The total pressure of the mixture is 450 kPa450 \text{ kPa}450 kPa. Calculate the value of the equilibrium constant, KpK_{\text{p}}Kp, for this reaction at temperature TTT, and state its units.