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The reaction system POCL3(g) -><- POCL(g) + Cl2(g) is at equilibrium. Which of the following statements...

The reaction system POCL3(g) -><- POCL(g) + Cl2(g) is at equilibrium. Which of the following statements describes the behavior of the system if POCL is added to the container?

A) The reverse reaction will proceed to establish equilibrium.

B) The partial pressure of cholrine will increase while the partial pressure of POCL decreases.

C) The partial pressure of chlorine remains steady while the partal pressures of POCL3 and POCL increase

D The forward reaction will proceed to establish equilibrium.

E) The partial pressures of POCL3 and POCL will remain steady while the partial pressure of clhorine increases.

Please explain how and why you got your answer

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Answer #1

Ans is A

explanation

Okay. So, pretend the equation's a see-saw, and it's perfectly balanced between reactants and products, right?

But then you just added some POCl, so the products side is heavier. You need to get rid of the products you just added to re-balance it.

So what the reaction will do is proceed backwards to both produce more reactants (POCl3) AND reduce the amount of POCl on the Products side. Essentially, it splits up the POCl you added so that the reactants side of the see-saw has some extra weight to compensate for the weight you added to the products.

In fewer words, the equation will react away the extra POCl, turning it into POCl3 to re-balance itself.

I believe the answer is A.

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