Nitrogen can react with hydrogen to produce ammonia in a reversible reaction: N2(g)+3H2(g)⇌2NH3(g)ΔH∘=−92 kJ mol−1\text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g}) \quad \Delta H^\circ = -92\text{ kJ mol}^{-1}N2(g)+3H2(g)⇌2NH3(g)ΔH∘=−92 kJ mol−1
State how a graph of partial pressure against time would show that this reaction mixture has reached equilibrium.
A 0.300 mol0.300\text{ mol}0.300 mol sample of nitrogen is mixed with hydrogen in a 1:31:31:3 mole ratio and allowed to reach equilibrium in a sealed flask at temperature TTT. At equilibrium, the mixture contains 0.180 mol0.180\text{ mol}0.180 mol of nitrogen. The total pressure of this mixture is 1.60×104 kPa1.60 \times 10^4\text{ kPa}1.60×104 kPa.
Calculate the partial pressure, in kPakPakPa, of hydrogen in the equilibrium mixture.
Give an expression for the equilibrium constant (KpK_pKp) for this reaction and state its units.
Some more nitrogen is added to the equilibrium mixture. The new mixture is allowed to reach equilibrium at temperature TTT. State the effect, if any, on the partial pressure of ammonia and on the value of KpK_pKp.
State the effect, if any, of the addition of a catalyst on the value of KpK_pKp for this equilibrium. Explain your answer.