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Chapter 14: Problem 51

List four factors that can shift the position of an equilibrium. Only one of these factors can alter the value of the equilibrium constant. Which one is it?

Short Answer

Expert verified
The four factors that can shift the position of an equilibrium are changes in concentration, pressure, temperature, and the addition of a catalyst. However, only changes in temperature can alter the value of the equilibrium constant.

Step by step solution

01

Identifying the four factors

The four primary factors that can affect the position of an equilibrium include: Changes in concentration, Changes in temperature, Changes in pressure, Addition of a catalyst.
02

Analyzing each factor: Concentration

Changes in the concentration of either reactants or products can shift the position of the equilibrium according to Le Chatelier's principle. If the concentration of a reactant is increased, the system will shift to the right, favoring the forward reaction and thus producing more products. Similarly, if the concentration of a product is increased, the system will shift to the left, favoring the reverse reaction and producing more reactants. However, changes in concentration do not influence the equilibrium constant.
03

Analyzing each factor: Pressure

Changes in pressure can also shift the position of the equilibrium, especially for reactions involving gases. Increasing the pressure results in the system shifting in the direction that reduces the pressure, i.e., towards the side with fewer gas molecules (lower volume). Reducing the pressure shifts the equilibrium towards the side with more gas molecules (higher volume). Still, changes in pressure do not affect the equilibrium constant.
04

Analyzing each factor: Temperature

Changes in temperature can shift the equilibrium and also change the value of the equilibrium constant, making this the answer to the second part of the question. An increase in temperature for an endothermic reaction (one that absorbs heat) will shift the equilibrium towards the products and increase K. On the other hand, for an exothermic reaction (a reaction that releases heat), an increase in temperature will shift the equilibrium towards the reactants and decrease K.
05

Analyzing each factor: Catalyst

The addition of a catalyst only speeds up the rate at which equilibrium is reached. It does not shift the position of the equilibrium nor does it change the value of the equilibrium constant.

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Most popular questions from this chapter

The equilibrium constant \(K_{P}\) for the reaction $$2 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g)$$ is \(2 \times 10^{-42}\) at \(25^{\circ} \mathrm{C}\). (a) What is \(K_{\mathrm{c}}\) for the reaction at the same temperature? (b) The very small value of \(K_{P}\) (and \(K_{\mathrm{c}}\) ) indicates that the reaction overwhelmingly favors the formation of water molecules. Explain why, despite this fact, a mixture of hydrogen and oxygen gases can be kept at room temperature without any change.

The equilibrium constant \(K_{\mathrm{c}}\) for the reaction $$\mathrm{H}_{2}(g)+\mathrm{CO}_{2}(g) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}(g)$$ is 4.2 at \(1650^{\circ} \mathrm{C}\). Initially \(0.80 \mathrm{~mol} \mathrm{H}_{2}\) and \(0.80 \mathrm{~mol}\) \(\mathrm{CO}_{2}\) are injected into a 5.0 - \(\mathrm{L}\) flask. Calculate the concentration of each species at equilibrium.

Pure nitrosyl chloride (NOCl) gas was heated to \(240^{\circ} \mathrm{C}\) in a \(1.00-\mathrm{L}\) container. At equilibrium the total pressure was 1.00 atm and the \(\mathrm{NOCl}\) pressure was 0.64 atm. $$2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g)$$ (a) Calculate the partial pressures of \(\mathrm{NO}\) and \(\mathrm{Cl}_{2}\) in the system. (b) Calculate the equilibrium constant \(K_{P}\).

The vapor pressure of mercury is \(0.0020 \mathrm{mmHg}\) at \(26^{\circ} \mathrm{C}\). (a) Calculate \(K_{\mathrm{c}}\) and \(K_{P}\) for the process \(\mathrm{Hg}(l) \rightleftharpoons \mathrm{Hg}(g) .\) (b) A chemist breaks a thermometer and spills mercury onto the floor of a laboratory measuring \(6.1 \mathrm{~m}\) long, \(5.3 \mathrm{~m}\) wide, and \(3.1 \mathrm{~m}\) high. Calculate the mass of mercury (in grams) vaporized at equilibrium and the concentration of mercury vapor in \(\mathrm{mg} / \mathrm{m}^{3}\). Does this concentration exceed the safety limit of \(0.05 \mathrm{mg} / \mathrm{m}^{3} ?\) (Ignore the volume of furniture and other objects in the laboratory.)

Define equilibrium. Give two examples of a dynamic equilibrium.
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