State one large scale use of hydrogen in the chemical industry.
Using the information above, state and explain how the equilibrium position changes when the applied pressure is increased. The reaction is: $\text{CH}_4(g) + \text{H}_2\text{O}(g) \rightleftharpoons \text{CO}(g) + 3\text{H}_2(g)$, $\Delta H = +206\,\text{kJ mol}^{-1}$.
Using the information above, state and explain how the equilibrium position changes when the equilibrium is cooled. The reaction is: $\text{CH}_4(g) + \text{H}_2\text{O}(g) \rightleftharpoons \text{CO}(g) + 3\text{H}_2(g)$, $\Delta H = +206\,\text{kJ mol}^{-1}$.
What effect will increasing the pressure have on the rate of reaction? Explain your answer.
Give the expression for $K_c$ for the reaction: $\text{CO}(g) + \text{H}_2\text{O}(g) \rightleftharpoons \text{CO}_2(g) + \text{H}_2(g)$. It is given that $K_c = 6.40 \times 10^{-1}$ at $1100\,\text{K}$.
Calculate the number of moles of each substance present in the equilibrium mixture at $1100\,\text{K}$. A mixture containing $0.40$ mol of $\text{CO}$, $0.40$ mol of $\text{H}_2\text{O}$, $0.20$ mol of $\text{CO}_2$ and $0.20$ mol of $\text{H}_2$ was placed in a $1\,\text{dm}^3$ flask and left until equilibrium was reached. Reaction: $\text{CO}(g) + \text{H}_2\text{O}(g) \rightleftharpoons \text{CO}_2(g) + \text{H}_2(g)$.