Chapter 23, Problem 23.26P

Interpretation Introduction

Interpretation:

Value of ${\text{ΔG}}_{rxn}^o$ at $527°C$ has to be calculated. The direction in which the reaction is spontaneous when $\left[CO\right]=\left[C{l}_2\right]=\left[COC{l}_2\right]=1.00\text{ M}$ has to be identified. Also, the value of ${\text{ΔG}}_{rxn}$ and direction in which the reaction is spontaneous has to be determined when $\left[CO\right]=\left[C{l}_2\right]=0.010\text{ M}$ and $\left[COC{l}_2\right]=1.00\text{ M}$.

Concept Introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by $\Delta G$. Value of $\Delta G_{rxn}^o$ is determined as follows,

  ${\text{ΔG}}_{rxn}^o=-\text{RT}\text{ln K}$

The formula of ${\text{ΔG}}_{\text{rxn}}$ in is given below,

    ${\text{ΔG}}_{rxn}=\text{RT}\text{ln }\left(\frac{{\text{Q}}_c}{K_c}\right)$

If $Q_c>{\text{ K}}_c$ then the reaction is spontanous in backward reaction (from right to left).

If $Q_c{\text{< K}}_c$ then the reaction is spontanous in forward reaction (from left to right).

If $Q_c={\text{ K}}_c$ then the reaction will be at equilibrium.