IB Chemistry HL 3.2.14 Gibbs Energy and Cell Potential Question Bank

Practise IB Chemistry HL 3.2.14 with questions linking ΔG° = −nFE°cell to electron transfer and spontaneity.

Exam points

derive n from electrons transferred in the balanced overall redox equation
apply ΔG° = −nFE°cell with volts and the Faraday constant using consistent units
connect positive E°cell with negative ΔG° and thermodynamic spontaneity

[Maximum number: 2]

A standard hydrogen electrode is connected to a copper-copper(II) nitrate half-cell.

Calculate the standard Gibbs free energy of the cell, in $\mathrm{kJ} \mathrm{mol}^{-1}$ . Use sections 1, 2 and 24 of the data booklet.

$\begin{aligned} \mathrm{n}=2 \text { « }-2(96500)(0.34)=»-65620 \text { «J mol }{ }^{-1} » /-65.6 \text { « } \mathrm{kJ} \mathrm{~mol}^{-1} » \vee \end{aligned}$

Answer must be negative

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3.2.14 (HL)—Gibbs energy and cell potential question 1