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Chapter 14: Problem 57

Consider the equilibrium $$2 \mathrm{I}(g) \rightleftharpoons \mathrm{I}_{2}(g)$$ What would be the effect on the position of equilibrium of (a) increasing the total pressure on the system by decreasing its volume; (b) adding gaseous I \(_{2}\) to the reaction mixture; and (c) decreasing the temperature at constant volume?

Short Answer

Expert verified
The changes will have the following effects: (a) Increasing the pressure by decreasing the volume shifts equilibrium to the right, producing more I\( _{2} \). (b) Adding gaseous I\( _{2} \) shifts the equilibrium to the left, producing more I(g). (c) Decreasing the temperature shifts the equilibrium to the right, producing more I\( _{2} \).

Step by step solution

01

Effects of increasing pressure

According to Le Chatelier’s principle, when the pressure of a system at equilibrium is increased, the system will shift in the direction that reduces the number of moles of gas. For this reaction, the forward reaction produces fewer moles of gas (1 mole I\( _{2} \)) compared to the reverse reaction (2 moles I). Therefore, when the pressure is increased by reducing volume, the reaction will shift to the right (making more I\( _{2} \)).
02

Effects of adding gaseous I\( _{2} \)

Le Chatelier’s principle also predicts that if the concentration of a product of a reaction at equilibrium is increased, then the reaction will shift in the direction that consumes that product, to minimize the change. Hence, if more I\( _{2} \) is added, the reaction will shift in the reverse direction, producing more I(g).
03

Effects of decreasing temperature

According to Le Chatelier's principle, if a system at equilibrium is subjected to a decrease in temperature, the system will shift in the direction that absorbs heat. In this case, since the given reaction is exothermic (heat is a product), if the temperature is decreased at constant volume, the system will shift to the right to produce more heat, thereby producing more I\( _{2} \).

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Most popular questions from this chapter

One mole of \(\mathrm{N}_{2}\) and three moles of \(\mathrm{H}_{2}\) are placed in a flask at \(375^{\circ} \mathrm{C}\). Calculate the total pressure of the system at equilibrium if the mole fraction of \(\mathrm{NH}_{3}\) is \(0.21 .\) The \(K_{P}\) for the reaction is \(4.31 \times 10^{-4}\).

The following equilibrium constants were determined at \(1123 \mathrm{~K}\) $$\begin{array}{ll}\mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g) & K_{P}^{\prime}=1.3 \times 10^{14} \\\\\mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{COCl}_{2}(g) & K_{P}^{\prime \prime}=6.0 \times 10^{-3}\end{array}$$ Write the equilibrium constant expression \(K_{P}\), and calculate the equilibrium constant at \(1123 \mathrm{~K}\) for $$\mathrm{C}(s)+\mathrm{CO}_{2}(g)+2 \mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{COCl}_{2}(g)$$

The equilibrium constant \(K_{P}\) for the reaction $$\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)$$ is 1.05 at \(250^{\circ} \mathrm{C}\). The reaction starts with a mixture of \(\mathrm{PCl}_{5}, \mathrm{PCl}_{3},\) and \(\mathrm{Cl}_{2}\) at pressures \(0.177 \mathrm{~atm},\) 0.223 atm, and 0.111 atm, respectively, at \(250^{\circ} \mathrm{C}\). When the mixture comes to equilibrium at that temperature, which pressures will have decreased and which will have increased? Explain why.

Eggshells are composed mostly of calcium carbonate \(\left(\mathrm{CaCO}_{3}\right)\) formed by the reaction $$\mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{3}^{2-}(a q) \rightleftharpoons \mathrm{CaCO}_{3}(s)$$ The carbonate ions are supplied by carbon dioxide produced as a result of metabolism. Explain why eggshells are thinner in the summer when the rate of panting by chickens is greater. Suggest a remedy for this situation.

When a gas was heated under atmospheric conditions, its color deepened. Heating above \(150^{\circ} \mathrm{C}\) caused the color to fade, and at \(550^{\circ} \mathrm{C}\) the color was barely detectable. However, at \(550^{\circ} \mathrm{C},\) the color was partially restored by increasing the pressure of the system. Which of the following best fits the above description? Justify your choice. (a) A mixture of hydrogen and bromine, (b) pure bromine, (c) a mixture of nitrogen dioxide and dinitrogen tetroxide. (Hint: Bromine has a reddish color and nitrogen dioxide is a brown gas. The other gases are colorless.)
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