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Chapter 19: Problem 73

Explain qualitatively how \(\Delta G\) changes for each of the following reactions as the partial pressure of \(\mathrm{O}_{2}\) is increased: (a) \(2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)\) (b) \(2 \mathrm{H}_{2} \mathrm{O}_{2}(l) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)\) (c) \(2 \mathrm{KClO}_{3}(s) \longrightarrow 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)\)

Short Answer

Expert verified
For each reaction: (a) Increasing the partial pressure of O鈧� shifts the reaction towards the right side, making 螖G more negative. (b) Increasing the partial pressure of O鈧� shifts the reaction towards the left side, making 螖G less negative or more positive. (c) Increasing the partial pressure of O鈧� shifts the reaction towards the left side, making 螖G less negative or more positive.

Step by step solution

01

(a) Reaction 1: \(2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)\)

(For reaction 1, increasing the partial pressure of O鈧� would cause the reaction to shift towards the right side, i.e., towards the formation of CO鈧� gas. This is because, an increase in the partial pressure of O鈧�, a reactant, would result in an increase in the rate of the forward reaction. This would help maintain equilibrium and hence, 螖G would become more negative as more reactants are converted into products (CO鈧�).)
02

(b) Reaction 2: \(2 \mathrm{H}_{2} \mathrm{O}_{2}(l) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)\)

(For reaction 2, increasing the partial pressure of O鈧� would cause the reaction to shift towards the left side, i.e., towards the formation of hydrogen peroxide (H鈧侽鈧�). This is because an increase in the partial pressure of O鈧�, a product, would result in an increase in the rate of the reverse reaction. This would help maintain equilibrium and hence, 螖G would become less negative or more positive as more products are converted back to reactants (H鈧侽鈧�).)
03

(c) Reaction 3: \(2 \mathrm{KClO}_{3}(s) \longrightarrow 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)\)

(For reaction 3, increasing the partial pressure of O鈧� would cause the reaction to shift towards the left side, i.e., towards the formation of potassium chlorate (KClO鈧�). This is because an increase in the partial pressure of O鈧�, a product, would result in an increase in the rate of the reverse reaction. This would help maintain equilibrium and hence, 螖G would become less negative or more positive as more products are converted back to reactants (KClO鈧�).)

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Most popular questions from this chapter

Which of the following processes are spontaneous: (a) the melting of ice cubes at \(10^{\circ} \mathrm{C}\) and 1 atm pressure; (b) separating a mixture of \(\mathrm{N}_{2}\) and \(\mathrm{O}_{2}\) into two separate samples, one that is pure \(\mathrm{N}_{2}\) and one that is pure \(\mathrm{O}_{2}\); (c) alignment of iron filings in a magnetic field; (d) the reaction of sodium metal with chlorine gas to form sodium chloride; (e) the dissolution of \(\mathrm{HCl}(g)\) in water to form concentrated hydrochloric acid?

Using data from Appendix \(C\), calculate \(\Delta G^{\circ}\) for the following reactions. lndicate whether each reaction is spontaneous under standard conditions. (a) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)\) (b) \(\mathrm{NO}_{2}(g)+\mathrm{N}_{2} \mathrm{O}(g) \longrightarrow 3 \mathrm{NO}(g)\) (c) \(6 \mathrm{Cl}_{2}(g)+2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s) \longrightarrow 4 \mathrm{FeCl}_{3}(s)+3 \mathrm{O}_{2}(g)\) (d) \(\mathrm{SO}_{2}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{S}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)\)

In each of the following pairs, which compound would you expect to have the higher standard molar entropy: (a) \(\mathrm{C}_{2} \mathrm{H}_{2}(g)\) or \(\mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{~g})\); (b) \(\mathrm{CO}_{2}(g)\) or \(\mathrm{CO}(g) ?\) Explain.

(a) Give two examples of endothermic processes that are spontaneous. (b) Give an example of a process that is spontaneous at one temperature but nonspontaneous at a different temperature.

Indicate whether \(\Delta G\) increases, decreases, or does not change when the partial pressure of \(\mathrm{H}_{2}\) is increased in each of the following reactions: (a) \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)\) (b) \(2 \mathrm{HBr}(g) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g)\) (c) \(2 \mathrm{H}_{2}(g)+\mathrm{C}_{2} \mathrm{H}_{2}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{6}(g)\)
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