IB Chemistry HL 3.2.13 Hl Standard Cell Potential E Cell Questions

Use real HL exam questions to calculate E°cell from reduction potentials, choose cell direction and predict whether redox reactions are spontaneous.

Exam points

Select the cathode reduction and anode oxidation directions for a spontaneous cell from the relative half-cell potentials.
Calculate E°cell as E°cathode − E°anode using tabulated standard reduction potentials, without scaling potentials when balancing equations.
Use a positive E°cell to predict standard-state spontaneity and identify feasible overall redox reactions and balanced equations.

[Maximum number: 1]

Magnesium is a group 2 metal which exists as a number of isotopes and forms many compounds.

A magnesium half-cell, $\mathrm{Mg}(\mathrm{s}) / \mathrm{Mg}^{2+}(\mathrm{aq})$ , can be connected to a copper half-cell, $\mathrm{Cu}(\mathrm{s}) / \mathrm{Cu}^{2+}(\mathrm{aq})$ .

Determine the standard cell potential, in V, for the cell. Refer to section 24 of the data booklet.

$<+0.34 \mathrm{~V}-(-2.37 \mathrm{~V})=+>2.71$ «V»

All question bank results loaded

IB Chemistry HL 3.2.13 Hl Standard Cell Potential E Cell Questions question 1