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Question 210 pts Predict the effect if the partial pressure of PCl5(g) is increased using the...

Question 210 pts

Predict the effect if the partial pressure of PCl5(g) is increased using the following equation.

PCl3(g) +Cl2(g)⟶ PCl5(g)

Group of answer choices

Shift right.

Shift left.

An increase in partial pressure of phosphorous trichloride and phosphorous pentachloride.

No effect.

A decrease in partial pressure of phosphorous trichloride and phosphorous pentachloride.

Solutions

Expert Solution

According to the Le Chatelier principle, if any changes are made to a reaction at equilibrium, the reaction will shift in a direction such that the effect of the change is nullified.

Therefore when the partial pressure of PCl5(g) is increased, the reaction will shift in a direction in which the partial pressure of PCl5(g) will decrease.

From the given chemical equation, if the reaction shifts to the right, more PCl5(g) is produced and more PCl3(g) and Cl2(g) are consumed. Hence the partial pressure of PCl5(g) will increase and the partial pressures of  PCl3(g) and Cl2(g) will decrease if the reaction shifts right.

If the reaction shifts to the left, more PCl5(g) is consumed and more PCl3(g) and Cl2(g) are produced. Hence the partial pressure of PCl5(g) will decrease and the partial pressures of  PCl3(g) and Cl2(g) will increase if the reaction shifts left.

Since the system wants to the decrease the partial pressure of PCl5(g) , the reaction will shift to the left.

Therefore the correct answer is the second option, that is:

Shift left.

queen_honey_blossom answered 2 years ago
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