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Chapter 38: Problem 8

Explain why the reaction quotient is useful.

Short Answer

Expert verified
As a chemical tool, the reaction quotient (Q) is vital because it allows the prediction of the direction in which a reaction will proceed to reach equilibrium. If Q>K, the reaction proceeds in the reverse direction; if Q<K, it goes in the forward direction; and if Q=K, the reaction is at equilibrium.

Step by step solution

01

Define Reaction Quotient

The reaction quotient (Q) is a measure of the relative quantities of reactants and products present in a reaction at a given time. It is calculated in the same way as the equilibrium constant, but the concentrations used in the calculation are not necessarily equilibrium concentrations.
02

Explain Function of Reaction Quotient

The reaction quotient serves as a tool for determining the direction a reaction will proceed to reach equilibrium. If the reaction quotient Q is greater than the equilibrium constant (K), the reaction will proceed in the reverse direction, converting products into reactants to reach equilibrium. Conversely, if Q is less than K, the reaction will proceed in the forward direction, converting reactants into products until equilibrium is achieved.
03

Describe Relationship between Reaction Quotient and Equilibrium Constant

If the reaction quotient Q equals the equilibrium constant K, the reaction is at equilibrium, which means that the rate of the forward reaction equals the rate of the reverse reaction, and the concentrations of the reactants and products remain constant.

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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.

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?

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.

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.
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