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Chapter 38: 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 injected into the box? Explain your reasoning.

Short Answer

Expert verified
The number of moles of \(\mathrm{PCl}_{3}\) will increase after injecting \(\mathrm{Cl}_{2}\) gas into the box.

Step by step solution

01

Analyze CTQ 13

Review the initial equilibrium state before the addition of the \(\mathrm{Cl}_{2}\) gas. Refer back to CTQ 13 to find out the equilibrium constants and concentrations of \(\mathrm{PCl}_{3}\) and \(\mathrm{Cl}_{2}\) before any changes. This will give a baseline from which to observe any shifts.
02

Apply Le Chatelier's Principle

After the \(\mathrm{Cl}_{2}\) gas is added, the concentration of \(\mathrm{Cl}_{2}\) will increase. According to Le Chatelier's principle, the system will try to alleviate this stress by shifting to reduce the concentration of \(\mathrm{Cl}_{2}\) and restore equilibrium. This will involve the forward reaction, hence increasing the quantity of \(\mathrm{PCl}_{3}\).
03

Conclude the Outcome

The addition of \(\mathrm{Cl}_{2}\) gas will cause the equilibrium to shift to the left, increasing the concentration of \(\mathrm{PCl}_{3}\). Observing the change in \(\mathrm{PCl}_{3}\) will confirm this effect.

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Most popular questions from this chapter

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 \(\mathrm{PCl}_{5}\) gas is suddenly injected into the box? Explain your reasoning.

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.

In general, how does the rate of the forward reaction \((\mathrm{Y} \rightarrow \mathrm{Z})\) at equilibrium compare to the rate of the reverse reaction \((\mathrm{Z} \rightarrow \mathrm{Y})\) at equilibrium?

Explain why the reaction quotient is useful.
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