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Chapter 16: Q16.4-67E (page 913)

What happens to \({\bf{\Delta G}}_{{\bf{298}}}^{\bf{^\circ }}\) (becomes more negative or more positive) for the following chemical reactions when the partial pressure of oxygen is increased?

(a) \({\bf{S(s) + }}{{\bf{O}}_{\bf{2}}}{\bf{(g)}} \to {\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\)

(b) \({\bf{2S}}{{\bf{O}}_{\bf{2}}}{\bf{(g) + }}{{\bf{O}}_{\bf{2}}}{\bf{(g)}} \to {\bf{S}}{{\bf{O}}_{\bf{3}}}{\bf{(g)}}\)

(c) \({\bf{HgO(s)}} \to {\bf{Hg(l) + }}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\)

Short Answer

Expert verified
  1. As the partial pressure of oxygen is increased the ratio of pressures decreases which would in effect decrease the value of \(\Delta G\) and make it more negative.
  2. As the partial pressure of oxygen is increased the ratio of pressures decreases which would in effect decrease the value of \(\Delta G\) and make it more negative.
  3. As the partial pressure of oxygen is increased the value of \(\ln \left( {{{\rm{P}}_{{\rm{O}}2}}} \right)\) will also increase which would in effect increase the value of \(\Delta G\) and make it more positive.

Step by step solution

01

Define free energy change

The free energy change is related to the partial pressures of the reactants and products through the following equation:

\(\Delta {\rm{G}} = \Delta {{\rm{G}}^0} + {\rm{RTln}}\left[ {\frac{{{\rm{ Partial pressure of products }}}}{{{\rm{ partial pressure of reactants }}}}} \right] - - - (1)\)

\(\Delta {{\rm{G}}^0} = \)standard free energy change

\({\rm{R}} = \) gas constant and \({\rm{T}} = \) temperature

02

a) Determine the decomposition reaction.

The given reaction is:

\({\rm{S}}({\rm{s}}) + {{\rm{O}}_2}(\;{\rm{g}}) \to {\rm{S}}{{\rm{O}}_2}(\;{\rm{g}})\)

Based on equation (1)

\(\Delta {\rm{G}} = \Delta {{\rm{G}}^0} + {\rm{RT}}\ln \left[ {\frac{{{{\rm{P}}_{{\rm{S}}{{\rm{O}}_2}}}}}{{{{\rm{P}}_{{{\rm{O}}_2}}}}}} \right]\)

As the partial pressure of oxygen is increased the ratio of pressures decreases which would in effect decrease the value of \(\Delta G\) and make it more negative.

03

b) Determine the free energy of the decomposition reaction.

The given reaction is:

\(2{\rm{S}}{{\rm{O}}_2}(\;{\rm{g}}) + {{\rm{O}}_2}(\;{\rm{g}}) \to 2{\rm{S}}{{\rm{O}}_3}(\;{\rm{g}})\)

Based on equation (1)

\(\Delta {\rm{G}} = \Delta {{\rm{G}}^0} + {\rm{RTln}}\left[ {\frac{{{\rm{P}}_{{\rm{S}}{{\rm{O}}_3}}^2}}{{{\rm{P}}_{{\rm{S}}{{\rm{O}}_2}}^2{{\rm{P}}_{{{\rm{O}}_2}}}}}} \right]\)

As the partial pressure of oxygen is increased the ratio of pressures decreases which would in effect decrease the value of \(\Delta G\) and make it more negative.

04

Determine the value of standard Gibbs free energy change

The given reaction is:

\({\rm{HgO}}({\rm{s}}) \to {\rm{Hg}}({\rm{l}}) + {{\rm{O}}_2}(\;{\rm{g}})\)

Based on equation (1)

\(\Delta {\rm{G}} = \Delta {{\rm{G}}^0} + {\rm{RTln}}\left[ {{{\rm{P}}_{{{\rm{O}}_2}}}} \right]\)

As the partial pressure of oxygen is increased the value of \(\ln \left( {{{\rm{P}}_{{\rm{O}}2}}} \right)\) will also increase which would in effect increase the value of \(\Delta G\) and make it more positive.

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Most popular questions from this chapter

Predict the sign of the enthalpy change for the following processes. Give a reason for your prediction.

(a) \({\bf{NaN}}{{\bf{O}}_{\bf{3}}}{\bf{(s)}} \to {\bf{N}}{{\bf{a}}^{\bf{ + }}}{\bf{(aq) + N}}{{\bf{O}}_{\bf{3}}}^{\bf{ - }}{\bf{(aq)}}\)

(b) the freezing of liquid water

(c) \({\bf{C}}{{\bf{O}}_{\bf{2}}}{\bf{(s)}} \to {\bf{C}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\)

(d) \({\bf{CaCO(s)}} \to {\bf{CaO(s) + C}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\)

Consider the decomposition of red mercury(II) oxide under standard state conditions.

\({\bf{2HgO(s, red )}} \to {\bf{2Hg(l) + }}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\)

(a) Is the decomposition spontaneous under standard state conditions?

(b) Above what temperature does the reaction become spontaneous?

In the laboratory, hydrogen chloride \({\bf{(HCl(g))}}\) and ammonia \(\left( {{\bf{N}}{{\bf{H}}_{\bf{3}}}{\bf{(g)}}} \right)\)often escape from bottles of their solutions and react to form the ammonium chloride\(\left( {{\bf{N}}{{\bf{H}}_{\bf{4}}}{\bf{Cl(s)}}} \right)\), the white glaze often seen on glassware. Assuming that the number of moles of each gas that escapes into the room is the same, what is the maximum partial pressure of \({\bf{HCl}}\) and \({\bf{N}}{{\bf{H}}_{\bf{3}}}\)in the laboratory at room temperature? (Hint: The partial pressures will be equal and are at their maximum value when at equilibrium.)

Describe how matter and/or energy is redistributed when you empty a canister of compressed air into a room.

Write conversion factors (as ratios) for the number of:

(a) yards in 1 meter

(b) liters in 1 liquid quart

(c) pounds in 1 kilogram
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