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Consider the following equilibrium: PCl5(g) <----> PCl3(g) + Cl2(g)

K= 0.040 What is the effect of increasing the pressure on this system at equilibrium?

Sagot :

Matalinesmarvin28idn

Answer:

Increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, which is the side with PCl3(g) and Cl2(g) in this case.

Explanation:

According to Le Chatelier’s Principle, if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. In this case, increasing the pressure will decrease the volume of the system, which will shift the equilibrium towards the side with fewer moles of gas. Since PCl5(g) has more moles of gas than PCl3(g) and Cl2(g) combined, increasing the pressure will favor the formation of PCl3(g) and Cl2(g) from PCl5(g), thus shifting the equilibrium towards the right side of the equation.

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