Consider the following equilibrium reaction for the synthesis of ammonia: N2(g)+3H2(g)⇌2NH3(g)\text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g})N2(g)+3H2(g)⇌2NH3(g)
Initially, 15.0 mol15.0 \text{ mol}15.0 mol of nitrogen and 38.0 mol38.0 \text{ mol}38.0 mol of hydrogen are placed in a sealed vessel. When the mixture reaches equilibrium at a certain temperature, it is found to contain 4.50 mol4.50 \text{ mol}4.50 mol of ammonia. Calculate the equilibrium amounts, in moles, of nitrogen and of hydrogen.
A different equilibrium mixture of nitrogen, hydrogen, and ammonia is established at a temperature TTT. At equilibrium, the mixture contains 3.15 mol3.15 \text{ mol}3.15 mol of nitrogen, 6.20 mol6.20 \text{ mol}6.20 mol of hydrogen, and 1.85 mol1.85 \text{ mol}1.85 mol of ammonia. The total pressure of the mixture is 850 kPa850 \text{ kPa}850 kPa. Calculate the value of the equilibrium constant, KpK_{\text{p}}Kp, for this reaction at temperature TTT, and state its units.