Chapter 17, Problem 17.58QE

(a)

Interpretation Introduction

Interpretation:

Free energy ($\Delta G°$) values has to be calculated for the given reaction.

  ${\text{N}}_2\left(\text{g}\right)\text{+}{\text{2H}}_2\left(\text{g}\right)\to {\text{N}}_{\text{2}}{H}_4\left(\text{l}\right)$

Concept Introduction:

The direction of spontaneous reaction:

• The forward reaction is spontaneous if the value of $\Delta G°$ is less than zero (negative).
• The reaction is at equilibrium if the value of $\Delta G°$ is zero.
• The forward reaction is non-spontaneous if the value of $\Delta G°$ is greater than zero (positive).

Free energy (Gibbs free energy) is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work.  The free energy is represented by the letter $\text{G}$.  All spontaneous process is associated with the decrease of free energy in the system.  The standard free energy change ${\text{(ΔG}}^{\text{°}}{}_{\text{rxn}})$ is the difference in free energy of the reactants and products in their standard state.

${\text{ΔG}}^{\text{°}}{}_{\text{rxn}}\text{=}\sum {\text{nΔG}}_{\text{f}}{}^{\text{°}}\text{(Products)-}\sum {\text{nΔG}}_{\text{f}}{}^{\text{°}}\text{(Reactants)}$

(b)

Interpretation Introduction

Interpretation:

Free energy ($\Delta G°$) values has to be calculated for the given reaction.

  ${\text{2H}}_{\text{2}}{\text{O}}_{\text{2}}\left(\text{l}\right)\to 2{\text{H}}_2\text{O}\left(l\right)+O_2\left(g\right)$

Concept Introduction:

Refer part (a).