Chapter 19: Q12P (page 662)

Calculate $Δ ε^{0'}$ and $Δ G^{0'}$ for the light reactions in plants, that is, the four-electron oxidation of H₂O by NADP⁺.

Short Answer

Expert verified

The values of ${ΔG}^{0'} = 438 kJ / mol$ and ${Δε}^{0'} = - 1.135 V$ .

Step by step solution

Obtaining values of Δε0'and ΔG0'

The values of ${Δε}^{0'}$ and ${ΔG}^{0'}$ are obtained from the figure of the Z-scheme photosynthesis.

Calculating the number of electrons

The value of ${Δε}^{0'}$ is found to be;

$\begin{matrix} {Δε}^{0'} = - 0.320 V - 0.815 V \\ = - 1.135 V \end{matrix}$

From the following reaction, the number of electrons is obtained;

$2 H_{2} O \to 4 H^{+} + O_{2} + 4 e^{-}$

Therefore, the number of electrons was found to be 4.

Calculating the change of free energy

$\begin{matrix} {ΔG}^{0'} = - {nFΔε}^{0'} \\ {ΔG}^{0'} = (- 4) \times (96, 485 C / mol) \times (- 1.135 V) \\ = 438000 J / mol \\ = 438 kJ / mol \end{matrix}$

Hence, the value of ${ΔG}^{0'} = 438 kJ / mol$ and ${Δε}^{0'} = - 1.135 V$ .

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Calculate $Δ ε^{0'}$ and $Δ G^{0'}$ for the light reactions in plants, that is, the four-electron oxidation of H₂O by NADP⁺.

Short Answer

Step by step solution

Obtaining values of Δε0'and ΔG0'

Calculating the number of electrons

Calculating the change of free energy

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Calculate Δε0'and ΔG0'for the light reactions in plants, that is, the four-electron oxidation of H2O by NADP+.

Short Answer

Step by step solution

Obtaining values of Δε0'and ΔG0'

Calculating the number of electrons

Calculating the change of free energy

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Biology Textbooks

Cells

Substance Exchange

Ecological Levels

Biological Organisms

Energy Transfers

Cell Communication

Study anywhere. Anytime. Across all devices.

Calculate $Δ ε^{0'}$ and $Δ G^{0'}$ for the light reactions in plants, that is, the four-electron oxidation of H₂O by NADP⁺.