Question

In the reaction between carbon monoxide, and chlorine, to give phosgene, what effect would an increase in temperature have on the equilibrium?

Answer 1

`CO(g) + Cl_2(g) stackrel("activated carbon")rarr COCl_2(g); DeltaH_"rxn"^@= −107.6 *kJ*mol^-1`

Explanation:

I take it this question relates to Le Chatelier's principle, and, therefore, I have included the thermodynamic parameters. The reaction as written is EXOTHERMIC, and we suspect, by the given principle, an increase in temperature would lead to the equilibrium going the other way, i.e. towards the REACTANT side to dissipate the excess heat.

Of course, industrially, where this reaction is performed in tonne quantities, a decrease in temperature might lead to an unacceptably low rate of reaction. The operating conditions of the reactor possibly balances rate (favoured with increased temperature) with position of the equilibrium, which of course we want to be TOWARDS the product. Capisce?