Consider the following exothermic reaction: C2H4 (g) + Cl2 (g) <-------> C2H4Cl2

Question

Consider the following exothermic reaction: C2H4 (g) + Cl2 (g) <-------> C2H4Cl2 (g) If you were a chemist trying to maximize the amount of C2H4Cl2 produced, which of the following might you try? Assume that the reaction mixture reaches equilibrium. a. increasing the reaction volume (Will maximize C2H4Cl2 or Will not maximize C2H4Cl2.) b. removing from the reaction mixture as it forms (Will maximize C2H4Cl2 or Will not maximize C2H4Cl2.) c. lowering the reaction temperature (Will maximize C2H4Cl2 or Will not maximize C2H4Cl2.) d. adding Cl2 (Will maximize C2H4Cl2 or Will not maximize C2H4Cl2.)

Explanation / Answer

the reaction is exothermic

the number of molecules reduces as the reaction proceeds forward

favourable conditions are low temperature and high pressure

a. increasing the volume will not maximise C2H4Cl2 as it will reduce the pressure shifting the equilibrium in the reverse direction

b. removing the reaction mixture as it forms will maximise C2H4Cl2 as it will keep the concentration of product at a minimum thus shifting the equilibrium forward

c. lowering the reaction will maximise C2H4Cl2 as the reaction is exothermic and excess heat needs to be removed

d. adding Cl2 will not maximise C2H4Cl2 as only one component increasing will not contribute to equilibrium shifting forward

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