A chemical plant synthesises various industrial gases using gas-phase catalytic reversible reactions.
The equations for two such reactions are: Reaction 1: CO(g)+Cl2(g)⇌COCl2(g)ΔH=−108 kJ/mol\text{CO(g)} + \text{Cl}_2\text{(g)} \rightleftharpoons \text{COCl}_2\text{(g)} \quad \Delta H = -108\text{ kJ/mol}CO(g)+Cl2(g)⇌COCl2(g)ΔH=−108 kJ/mol Reaction 2: 2SO2(g)+O2(g)⇌2SO3(g)ΔH=−197 kJ/mol2\text{SO}_2\text{(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{SO}_3\text{(g)} \quad \Delta H = -197\text{ kJ/mol}2SO2(g)+O2(g)⇌2SO3(g)ΔH=−197 kJ/mol
Assume that both reactions reach a position of dynamic equilibrium. (i) For Reaction 1, predict whether using a high or a low temperature would produce the higher equilibrium yield of carbonyl chloride, COCl2\text{COCl}_2COCl2. Give a reason for your choice.
For Reaction 2, predict whether using a high or a low pressure would produce the higher equilibrium yield of sulfur trioxide, SO3\text{SO}_3SO3. Give a reason for your choice.
A heterogeneous catalyst is introduced to increase the rate of both the forward and reverse reactions. Explain why this catalyst has no effect on the position of equilibrium.
Reaction 1 can be represented by a reaction profile diagram.
(i) Describe how to complete the profile diagram above to show the products of the reaction and the enthalpy change, ΔH\Delta HΔH.
Describe how to represent the activation energy, EaE_\text{a}Ea, for the forward reaction on this profile.
State the effect, if any, of the catalyst on the enthalpy change, ΔH\Delta HΔH, for the reaction.
