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Chapter 14: Problem 12

Give an example of a multiple equilibria reaction.

Short Answer

Expert verified
An example of a multiple equilibria reaction is the formation of sulfur trioxide and disulfur pentoxide from sulfur dioxide: \ 1. \[2SO2(g) + O2(g) \leftrightarrow 2SO3(g)\]\ 2. \(SO2(g) + SO3(g) \leftrightarrow S2O5(g)\)

Step by step solution

01

Understanding Multiple Equilibria

Multiple equilibria reactions refer to chemical reactions with more than one equilibrium point. This can occur when the products of a reaction can further react, creating a new equilibrium to coexist with the first.
02

Choose an Example

An example of a multiple equilibria reaction is conversion of sulfur dioxide (SO2) to sulfur trioxide (SO3) in the presence of a catalyst. This happens in two steps: \ 1. \[2SO2(g) + O2(g) \leftrightarrow 2SO3(g)\]\ 2. \(SO2(g) + SO3(g) \leftrightarrow S2O5(g)\) \ Each of these reactions is reversible, and under certain conditions will reach an equilibrium. However, since the product of the first reaction is a reactant in the second, the two equilibria are linked.

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Most popular questions from this chapter

A quantity of 1.0 mole of \(\mathrm{N}_{2} \mathrm{O}_{4}\) was introduced into an evacuated vessel and allowed to attain equilibrium at a certain temperature $$\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)$$ The average molar mass of the reacting mixture was \(70.6 \mathrm{~g} / \mathrm{mol} .\) (a) Calculate the mole fractions of the gases. (b) Calculate \(K_{P}\) for the reaction if the total pressure was 1.2 atm. (c) What would be the mole fractions if the pressure were increased to 4.0 atm by reducing the volume at the same temperature?

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.

The decomposition of ammonium hydrogen sulfide $$\mathrm{NH}_{4} \mathrm{HS}(s) \rightleftharpoons \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{~S}(g)$$ is an endothermic process. A 6.1589 -g sample of the solid is placed in an evacuated \(4.000-\mathrm{L}\) vessel at exactly \(24^{\circ} \mathrm{C}\). After equilibrium has been established, the total pressure inside is 0.709 atm. Some solid \(\mathrm{NH}_{4} \mathrm{HS}\) remains in the vessel. (a) What is the \(K_{P}\) for the reaction? (b) What percentage of the solid has decomposed? (c) If the volume of the vessel were doubled at constant temperature, what would happen to the amount of solid in the vessel?

What effect does an increase in pressure have on each of the following systems at equilibrium? The temperature is kept constant and, in each case, the reactants are in a cylinder fitted with a movable piston. (a) \(\mathrm{A}(s) \rightleftharpoons 2 \mathrm{~B}(s)\) (b) \(2 \mathrm{~A}(l) \rightleftharpoons \mathrm{B}(l)\) (c) \(\mathrm{A}(s) \rightleftharpoons \mathrm{B}(g)\) (d) \(\mathrm{A}(g) \rightleftharpoons \mathrm{B}(g)\) (e) \(\mathrm{A}(g) \rightleftharpoons 2 \mathrm{~B}(g)\)

Consider the gas-phase reaction $$2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{CO}_{2}(g)$$ Predict the shift in the equilibrium position when helium gas is added to the equilibrium mixture at (a) constant pressure and (b) constant volume.
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