Nitrosyl chloride decomposes reversibly in a closed vessel according to the following equation:
2NOCl(g)⇌2NO(g)+Cl2(g)ΔH=+76 kJ mol−1 2\text{NOCl(g)} \rightleftharpoons 2\text{NO(g)} + \text{Cl}_2\text{(g)} \quad \Delta H = +76\text{ kJ mol}^{-1} 2NOCl(g)⇌2NO(g)+Cl2(g)ΔH=+76 kJ mol−1A 4.20 mol4.20\text{ mol}4.20 mol sample of NOCl\text{NOCl}NOCl is sealed in a container of volume 12.5 dm312.5\text{ dm}^312.5 dm3 and heated to a constant temperature. When equilibrium is reached, the mixture is found to contain 0.84 mol0.84\text{ mol}0.84 mol of NOCl\text{NOCl}NOCl.
Calculate the amount, in moles, of NO\text{NO}NO and of Cl2\text{Cl}_2Cl2 in this equilibrium mixture.
Give an expression for KcK_cKc for this equilibrium.
Calculate the value of KcK_cKc at this temperature. State its units.
State and explain the effect of using a higher temperature on the equilibrium yield of nitric oxide (NO\text{NO}NO).
Nitrogen monoxide (NO\text{NO}NO) is an atmospheric pollutant formed in internal combustion engines. State one environmental problem caused by acid rain (which NO\text{NO}NO contributes to), and write a balanced chemical equation to show how NO\text{NO}NO is removed from exhaust emissions in a catalytic converter by reacting with carbon monoxide.
