Exercise 16.79 Consider the following exothermic reaction: C2H4 (g) Cl2(g) C2H4C

Question

Exercise 16.79 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. Part A increasing the reaction volume O Will maximize C2H4Cl2 O Will not maximize Co HAC1 Submit My Answers Give Up Part B removing C2H Cl from the reaction mixture as it forms o Will maximize C2HAC12 O Will not maximize C HACl Submit My Answers Give Up Part C lowering the reaction temperature o Will maximize C2HAC12 O Will not maximize C HACl

Explanation / Answer

C2H4(g) + Cl2(g) ----------C2H4Cl2 (g) - and exothermic reaction

PartA

As V increase, P decreases. Then the equilibrium shifts to the side where more gaseous moles present (to increase the P) .

Here reactants have more moles of gases thanproducts.

Thus increase in V shifts the qequilibirum towards lefts side so

WILL NOT maximise C2H4CL2

B) removal of C2H4Cl2

According to Le-chatlier principle, if the product is removed the equilibrium shift s in direction to increse its concentration.

Thus removela products shifts it right side so WILL maximise C2H4Cl2

C0 Exothermic reactions are favored at lower temperature, thus lowering temperature increases production of C2H4Cl2.

Will maximise C2H4Cl2

D0 If the reactant concentration is increased , forward reaction is favored.

So increasing/ adding more Cl2 WILL maximise C2H4Cl2.

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