1. The following reaction has achieved equilibrium. Predict the effect on the fo
ID: 813857 • Letter: 1
Question
1. The following reaction has achieved equilibrium. Predict the effect on the formation of phosphorous pentachloride (increase, decrease or no effect) for the stated changes to the system:
PCl3(g) + Cl2(g) <--> PCl5(g)
a) The concentration of phosphorous trichloride is increased.
b) The concentration of chlorine is decreased.
c) The volume of the container in which the reaction is taking place is suddenly made smaller.
d) The pressure of the system is increased by adding one atmosphere of gaseous nitrogen to the container.
--> Please Predict the effect on the formation of phosphorous pentachloride (increase, decrease or no effect) individually for a, b, c, and d. and if possible please include how you know what the effect would be. Thank you!!!
Explanation / Answer
The following reaction has achieved equilibrium. Predict the effect on the formation of phosphorous pentachloride (increase, decrease or no effect) for the stated changes to the system:
PCl3(g) + Cl2(g) = PCl5(g)
The volume of the container in which the reaction is taking place is suddenly made smaller and the pressure of the system is increased by adding one atmosphere of gaseous nitrogen to the container.
Answer
The euqilibrium shifts in a direction so as to oppose the change that has been produced.
increase in pressure shifts the equilibrium towards right as 2moles of gas give one mole of the other.
and the same applies when volume is decreased as volume is inversely proportional to pressure and thus decrease in volume implies increase in pressure at constant temperature.
and the answer to the question is : formation of phosphorous pentachloride increases.
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