Chapter 1: Q13P (page 21)

Calculate or the reactionat when the equilibrium concentrations are. Is the reaction exergonic or endergonic under standard conditions?

Short Answer

Expert verified

The standard free energy change for the reaction is ${ΔG}^{0'} = 5.703 {kJmol}^{- 1}$ .

Step by step solution

Given data

${ΔG}^{0'} = 5.703 kJmo l^{- 1} A + B \Leftrightarrow C + D$

Concentration of the reactants is $[A] = 10 μM; [B] = 15 μM;$

Concentration of the products is $[C] = 3 μM; [B] = 5 μM;$

Temperature, T=298 K

Calculating the standard free energy change

$\begin{array}{l} {ΔG}^{0'} = - {RTlnK}_{eq} \\ = - RTln \frac{[C] [D]}{[A] [B]} \end{array}$

On substituting the standard free energy change values

$\begin{array}{l} Δ G^{0'} = - 8.314 \times 298 \times \ln \frac{3 \times 5}{10 \times 15} \\ = - 2477.57 \times (\ln 1 - \ln 10) \\ = - 2477.57 \times - 2.302 \\ = 5703.37 k J m o l^{- 1} \\ Δ G^{0'} = 5.703 k J m o l^{- 1} \end{array}$

Therefore, the standard free energy change for the reaction is $\begin{array}{l} {ΔG}^{0'} = 5.703 {kJmol}^{- 1} \end{array}$ .

Hence, the reaction is nonspontaneous or endergonic at standard conditions.

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Calculate or the reactionat when the equilibrium concentrations are. Is the reaction exergonic or endergonic under standard conditions?

Short Answer

Step by step solution

Given data

Calculating the standard free energy change

On substituting the standard free energy change values

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