Some bond energies are provided. $\text{N} \equiv \text{N} = 944\ \text{kJ mol}^{-1}$ $\text{H} - \text{H} = 436\ \text{kJ mol}^{-1}$ Explain what is meant by the term bond energy.
Calculate a value for the $\text{N} - \text{H}$ bond energy from the data. Show your working.
The Boltzmann distribution for a mixture of nitrogen and hydrogen at $400\,^{\circ}\text{C}$ is shown. $E_a$ represents the activation energy for the reaction. On the same axes, sketch a second curve to show the Boltzmann distribution at a higher temperature.
With reference to the Boltzmann distribution, state and explain how increasing temperature affects the rate at which ammonia is produced.
State and explain the effect of increasing temperature on the yield of ammonia. Use Le Chatelier’s principle in your explanation.
At a pressure of $2.00 \times 10^7\ \text{Pa}$, $1.00\ \text{mol}$ of nitrogen, $\text{N}_2\text{(g)}$, was combined with $3.00\ \text{mol}$ of hydrogen, $\text{H}_2\text{(g)}$. The final equilibrium mixture contained $0.300\ \text{mol}$ of ammonia, $\text{NH}_3\text{(g)}$. Calculate the amounts, in mol, of $\text{N}_2\text{(g)}$ and $\text{H}_2\text{(g)}$ present in the equilibrium mixture.
Calculate the partial pressure of ammonia, $p_{\text{NH}_3}$, in the equilibrium mixture. Give your answer to three significant figures.
In a different equilibrium mixture, the partial pressures are shown below: $\text{N}_2\text{(g)}: 2.20 \times 10^6\ \text{Pa}$ $\text{H}_2\text{(g)}: 9.62 \times 10^5\ \text{Pa}$ $\text{NH}_3\text{(g)}: 1.40 \times 10^4\ \text{Pa}$ Write the expression for the equilibrium constant, $K_p$, for ammonia formation from nitrogen and hydrogen.
Calculate the value of $K_p$ for this reaction, and state its units.
This reaction is carried out again with the same starting amounts of nitrogen and hydrogen. The temperature is unchanged, but the container volume is smaller. State the effects, if any, of this change on the yield of ammonia and on the value of $K_p$.