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Chapter 40: Problem 15

Assume that the system is at equilibrium as determined in CTQ \(13 .\) What will happen to the number of moles of \(\mathrm{PCl}_{3}\) present if some \(\mathrm{Cl}_{2}\) gas is suddenly added to the box? Explain your reasoning.

Short Answer

Expert verified
The number of moles of PCl3 will decrease to counteract the sudden addition of Cl2 gas and restore equilibrium according to Le Chatelier’s principle.

Step by step solution

01

Understand Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In this scenario, the condition changing is the amount of Cl2 added to the system.
02

Evaluate the Impact of Increased Cl2 on the Equilibrium

The addition of Cl2 will cause the equilibrium to shift to the right (since it appears on the left of the equilibrium equation). This is an attempt by the system to decrease the concentration of the excess reactant, which is Cl2 in this case.
03

Determine the Effect on PCl3

Because the equilibrium is shifting to the right to consume the excess Cl2, there will be more reaction of PCl3 with Cl2. As a result, the number of moles of PCl3 will decrease.

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Most popular questions from this chapter

Consider a situation in which the reaction quotient, \(Q_{\mathrm{c}}\), for a given reaction is larger than the equilibrium constant, \(K_{\mathrm{c}}\). a) How must the value of \(\mathrm{Q}_{\mathrm{c}}\) change to reach equilibrium? b) Describe how the concentrations of reactants and/or the concentration of products must change to reach equlibrium.

Explain why the reaction quotient is useful.
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