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Chapter 15: Problem 61

Consider the following equilibrium for which \(\Delta H<0\) $$2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g)$$ How will each of the following changes affect an equilibrium mixture of the three gases: (a) \(\mathrm{O}_{2}(g)\) is added to the system; (b) the reaction mixture is heated; (c) the volume of the reaction vessel is doubled; (d) a catalyst is added to the mixture; (e) the total pressure of the system is increased by adding a noble gas; (f) \(\mathrm{SO}_{3}(g)\) is removed from the system?

Short Answer

Expert verified
(a) The reaction will shift to the right, forming more SO₃(g). (b) The equilibrium will shift to the left, favoring the formation of SO₂(g) and O₂(g). (c) The equilibrium will shift to the left, towards the formation of SO₂(g) and O₂(g). (d) Adding a catalyst does not change the position of the equilibrium. (e) The equilibrium is not affected by the addition of a noble gas. (f) The equilibrium will shift to the right, favoring the formation of SO₃(g) from SO₂(g) and O₂(g).

Step by step solution

01

(a) Effect of adding O₂(g)

When O₂(g) is added to the system, the equilibrium will shift to consume the added reactant and counteract the change. Therefore, the reaction will shift to the right, towards the formation of SO₃(g).
02

(b) Effect of heating the reaction mixture

Since the reaction is exothermic (ΔH < 0), increasing the temperature will shift the equilibrium to the endothermic side to counteract the heat, which is the reverse reaction, favoring the formation of SO₂(g) and O₂(g). The equilibrium will shift to the left.
03

(c) Effect of doubling the volume of the reaction vessel

Doubling the volume of the reaction vessel will decrease the partial pressure of all the gases involved. In order to counteract this change, the reaction will shift in the direction of the side with more gas molecules. The reaction has 3 gas molecules on the reactant side and 2 gas molecules on the product side, therefore the equilibrium will shift to the left, towards the formation of SO₂(g) and O₂(g).
04

(d) Effect of adding a catalyst to the mixture

Adding a catalyst to the mixture will not change the position of the equilibrium. A catalyst speeds up both forward and reverse reactions equally, allowing the system to reach equilibrium faster, but does not affect the equilibrium concentrations.
05

(e) Effect of increasing the total pressure by adding a noble gas

Adding a noble gas to the system increases the total pressure, but it does not participate in the reaction. Therefore, the partial pressures of the reactants and products remain unchanged, and the equilibrium is not affected by the addition of a noble gas.
06

(f) Effect of removing SO₃(g) from the system

When SO₃(g) is removed from the system, the equilibrium shifts to counteract the change and attempts to replace the removed product. Thus, the equilibrium will shift to the right, favoring the formation of SO₃(g) from SO₂(g) and O₂(g).

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Most popular questions from this chapter

A certain chemical reaction has \(K_{c}=1.5 \times 10^{6}\). Does this mean that at equilibrium there are \(1.5 \times 10^{6}\) times as many product molecules as reactant molecules? Explain.

A \(0.831-\mathrm{g}\) sample of \(\mathrm{SO}_{3}\) is placed in a 1.00 - \(\mathrm{L}\) container and heated to \(1100 \mathrm{~K}\). The \(\mathrm{SO}_{3}\) decomposes to \(\mathrm{SO}_{2}\) and \(\mathrm{O}_{2}\) : $$2 \mathrm{SO}_{3}(g) \rightleftharpoons 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g)$$ At equilibrium the total pressure in the container is \(1.300 \mathrm{~atm}\). Find the values of \(K_{p}\) and \(K_{c}\) for this reaction at \(1100 \mathrm{~K}\).

Consider \(4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \rightleftharpoons 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g),\) \(\Delta H=-904.4 \mathrm{~kJ} .\) How does each of the following changes affect the yield of \(\mathrm{NO}\) at equilibrium? Answer increase, decrease, or no change: (a) increase \(\left[\mathrm{NH}_{3}\right] ;(\mathbf{b})\) increase \(\left[\mathrm{H}_{2} \mathrm{O}\right] ;(\mathrm{c})\) decrease \(\left[\mathrm{O}_{2}\right]\) (d) decrease the volume of the container in which the reaction occurs; (e) add a catalyst; (f) increase temperature.

At \(1000 \mathrm{~K}, K_{p}=1.85\) for the reaction $$ \mathrm{SO}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{SO}_{3}(g) $$ (a) What is the value of \(K_{p}\) for the reaction \(\mathrm{SO}_{3}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) ?(\mathbf{b})\) What is the value of \(K_{p}\) for the reaction \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g)\) ? (c) What is the value of \(K_{c}\) for the reaction in part (b)?

For the equilibrium $$ \mathrm{PH}_{3} \mathrm{BCl}_{3}(s) \rightleftharpoons \mathrm{PH}_{3}(g)+\mathrm{BCl}_{3}(g) $$ \(K_{p}=0.052\) at \(60^{\circ} \mathrm{C}\). (a) Calculate \(K_{c}\) (b) After \(3.00 \mathrm{~g}\) of solid \(\mathrm{PH}_{3} \mathrm{BCl}_{3}\) is added to a closed \(1.500\) - \(\mathrm{L}\) vessel at \(60{ }^{\circ} \mathrm{C}\), the vessel is charged with \(0.0500 \mathrm{~g}\) of \(\mathrm{BCl}_{3}(\mathrm{~g})\). What is the equilibrium concentration of \(\mathrm{PH}_{3}\) ?
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