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Chapter 13: Problem 67

In which direction will the position of the equilibrium $$ 2 \mathrm{HI}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) $$ be shifted for each of the following changes? a. \(\mathrm{H}_{2}(g)\) is added. b. \(\mathrm{I}_{2}(g)\) is removed. c. \(\mathrm{HI}(g)\) is removed. d. In a rigid reaction container, some \(\operatorname{Ar}(g)\) is added. e. The volume of the container is doubled. f. The temperature is decreased (the reaction is exothermic).

Short Answer

Expert verified
a. The equilibrium will shift to the right. b. The equilibrium will shift to the right. c. The equilibrium will shift to the left. d. The equilibrium will not shift. e. The equilibrium will shift to the right. f. The equilibrium will shift to the right.

Step by step solution

01

Determine the effect of the change

Increasing the concentration of a reactant (H2) will cause the system to move towards the product side (to the right). Therefore, the equilibrium will shift to the right to minimize the effect of the added H2. #b. Removing I2(g)#
02

Determine the effect of the change

Decreasing the concentration of one of the products (I2) will cause the system to replenish the depleted product, thus shifting the equilibrium to the product side (to the right). #c. Removing HI(g)#
03

Determine the effect of the change

Decreasing the concentration of a reactant (HI) will cause the system to shift towards the reactants side (to the left) in order to minimize the effect and increase the concentration of HI. #d. Adding Ar(g) in a rigid container#
04

Determine the effect of the change

Adding an inert gas (Ar) that doesn't participate in the reaction, in a rigid container (at constant volume) will not cause a change in the partial pressures of the reactants or products. Therefore, the equilibrium will not shift. #e. Doubling the volume of the container#
05

Determine the effect of the change

Doubling the volume of the container results in a decrease in the partial pressure of all gases in the system. To minimize this effect, the equilibrium will shift in the direction that increases the number of moles of gas. In this case, the equilibrium will shift to the right (as there are 2 moles of HI for every mole of H2 and I2). #f. Decreasing the temperature (reaction is exothermic)#
06

Determine the effect of the change

If the reaction is exothermic, it releases heat as it proceeds towards the products. When the temperature is decreased, the system will try to minimize the effect by producing more heat. Consequently, the equilibrium will shift to the right, favoring the formation of products.

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Most popular questions from this chapter

Given \(K=3.50\) at \(45^{\circ} \mathrm{C}\) for the reaction $$ \mathrm{A}(g)+\mathrm{B}(g) \rightleftharpoons \mathrm{C}(g) $$ and \(K=7.10\) at \(45^{\circ} \mathrm{C}\) for the reaction $$ 2 \mathrm{~A}(g)+\mathrm{D}(g) \rightleftharpoons \mathrm{C}(g) $$ what is the value of \(K\) at the same temperature for the reaction $$ \mathrm{C}(g)+\mathrm{D}(g) \rightleftharpoons 2 \mathrm{~B}(g) $$ What is the value of \(K_{\mathrm{p}}\) at \(45^{\circ} \mathrm{C}\) for the reaction? Starting with \(1.50\) atm partial pressures of both \(\mathrm{C}\) and \(\mathrm{D}\), what is the mole fraction of \(\mathrm{B}\) once equilibrium is reached?

Ethyl acetate is synthesized in a nonreacting solvent (not water) according to the following reaction: \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}+\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH} \rightleftharpoons \mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{C}_{2} \mathrm{H}_{5}+\mathrm{H}_{2} \mathrm{O} \quad K=2.2\) \(\begin{array}{ll}\text { Acetic acid } & \text { Ethanol } & \text { Ethyl acetate }\end{array}\) For the following mixtures \((\mathrm{a}-\mathrm{d})\), will the concentration of \(\mathrm{H}_{2} \mathrm{O}\) increase, decrease, or remain the same as equilibrium is established? a. \(\left[\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{C}_{2} \mathrm{H}_{5}\right]=0.22 \mathrm{M},\left[\mathrm{H}_{2} \mathrm{O}\right]=0.10 \mathrm{M}\), \(\left[\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\right]=0.010 \mathrm{M},\left[\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right]=0.010 \mathrm{M}\) b. \(\left[\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{C}_{2} \mathrm{H}_{5}\right]=0.22 M,\left[\mathrm{H}_{2} \mathrm{O}\right]=0.0020 M\), \(\left[\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\right]=0.0020 \mathrm{M},\left[\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right]=0.10 \mathrm{M}\) c. \(\left[\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{C}_{2} \mathrm{H}_{5}\right]=0.88 \mathrm{M},\left[\mathrm{H}_{2} \mathrm{O}\right]=0.12 \mathrm{M}\), \(\left[\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\right]=0.044 M,\left[\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right]=6.0 \mathrm{M}\) d. \(\left[\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{C}_{2} \mathrm{H}_{5}\right]=4.4 \mathrm{M},\left[\mathrm{H}_{2} \mathrm{O}\right]=4.4 \mathrm{M}\), \(\left[\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\right]=0.88 \mathrm{M},\left[\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right]=10.0 \mathrm{M}\) e. What must the concentration of water be for a mixture with \(\left[\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{C}_{2} \mathrm{H}_{5}\right]=2.0 \mathrm{M},\left[\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\right]=0.10 \mathrm{M}\), and \(\left[\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right]\) \(=5.0 M\) to be at equilibrium? f. Why is water included in the equilibrium expression for this reaction?

In a study of the reaction $$ 3 \mathrm{Fe}(s)+4 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+4 \mathrm{H}_{2}(g) $$ at \(1200 \mathrm{~K}\) it was observed that when the equilibrium partial pressure of water vapor is \(15.0\) torr, that total pressure at equilibrium is \(36.3\) torr. Calculate the value of \(K_{\mathrm{p}}\) for this reaction at \(1200 \mathrm{~K}\). (Hint: Apply Dalton's law of partial pressures.)

The equilibrium constant is \(0.0900\) at \(25^{\circ} \mathrm{C}\) for the reaction $$ \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{Cl}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{HOCl}(g) $$ For which of the following sets of conditions is the system at equilibrium? For those which are not at equilibrium, in which direction will the system shift? a. \(P_{\mathrm{H}_{2} \mathrm{O}}=1.00 \mathrm{~atm}, P_{\mathrm{Cl}_{2} \mathrm{O}}=1.00 \mathrm{~atm}, P_{\mathrm{HOCl}}=1.00 \mathrm{~atm}\) b. \(P_{\mathrm{H}_{2} \mathrm{O}}=200 .\) torr, \(P_{\mathrm{Cl}_{2} \mathrm{O}}=49.8\) torr, \(P_{\mathrm{HOCl}}=21.0\) torr c. \(P_{\mathrm{H}_{2} \mathrm{O}}=296\) torr, \(P_{\mathrm{Cl}_{2} \mathrm{O}}=15.0\) torr, \(P_{\mathrm{HOCl}}=20.0\) torr

Novelty devices for predicting rain contain cobalt(II) chloride and are based on the following equilibrium: $$ \underset{\text { Purple }}{\mathrm{CoCl}_{2}(s)}+6 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \underset{\text { Pink }}{\mathrm{CoCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}(s)} $$ What color will such an indicator be if rain is imminent?
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