standard cell potential $(E_{\text{cell}}^{^\circ})$

the cell potential when all reactants and products are in their standard states (1 bar or 1 atm or gases; 1 M for solutes), usually at 298.15 K

standard hydrogen electrode (SHE)

half-cell based on hydrogen ion production, assigned a potential of exactly 0 V under standard state conditions, used as the universal reference for measuring electrode potential

standard electrode potential ($(E_X^{^\circ})$)

electrode potential measured under standard conditions (1 bar or 1 atm for gases; 1 M for solutes) usually at 298.15 K

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Chemistry 2e · 17.3 Electrode and Cell Potentials

Electrode and Cell Potentials: practice problems

3 problems from the book, with its answers. Check your working, or have any of them explained to you on the whiteboard.

Exercises 21
Calculate the standard cell potential for each reaction below, and note whether the reaction is spontaneous under standard state conditions.
(a) $Mg (s) + Ni^{2 +} (a q) ⟶ Mg^{2 +} (a q) + Ni (s)$
(b) $2 Ag^{+} (a q) + Cu (s) ⟶ Cu^{2 +} (a q) + 2Ag (s)$
(c) $Mn (s) + Sn(NO_{3})_{2} (a q) ⟶ Mn(NO_{3})_{2} (a q) + Sn (s)$
(d) $3 Fe(NO_{3})_{2} (a q) + Au(NO_{3})_{3} (a q) ⟶ 3Fe(NO_{3})_{3} (a q) + Au (s)$
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Exercises 23
Write the balanced cell reaction for the cell schematic below, calculate the standard cell potential, and note whether the reaction is spontaneous under standard state conditions.
$Cu (s) │ Cu^{2 +} (a q) ║ Au^{3 +} (a q) │ Au (s)$
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Exercises 25
Determine the cell reaction and standard cell potential at 25 °C for a cell made from an anode half-cell containing a cadmium electrode in 1 M cadmium nitrate and a cathode half-cell consisting of an aluminum electrode in 1 M aluminum nitrate solution. Is the reaction spontaneous at standard conditions?
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Key terms · 3

standard cell potential $(E_{\text{cell}}^{^\circ})$: the cell potential when all reactants and products are in their standard states (1 bar or 1 atm or gases; 1 M for solutes), usually at 298.15 K
standard hydrogen electrode (SHE): half-cell based on hydrogen ion production, assigned a potential of exactly 0 V under standard state conditions, used as the universal reference for measuring electrode potential
standard electrode potential ($(E_X^{^\circ})$): electrode potential measured under standard conditions (1 bar or 1 atm for gases; 1 M for solutes) usually at 298.15 K

Learn 17.3 on the whiteboard

The tutor teaches the whole section, drawing it out step by step and answering your questions as you go.

Read 17.3 in the textbook · This section on openstax.org

Electrode and Cell Potentials: practice problems

3 problems from the book, with its answers. Check your working, or have any of them explained to you on the whiteboard.

Exercises 21

Calculate the standard cell potential for each reaction below, and note whether the reaction is spontaneous under standard state conditions.

(a) $Mg (s) + Ni^{2 +} (a q) ⟶ Mg^{2 +} (a q) + Ni (s)$

(b) $2 Ag^{+} (a q) + Cu (s) ⟶ Cu^{2 +} (a q) + 2Ag (s)$

(d) $3 Fe(NO_{3})_{2} (a q) + Au(NO_{3})_{3} (a q) ⟶ 3Fe(NO_{3})_{3} (a q) + Au (s)$

Exercises 23

Write the balanced cell reaction for the cell schematic below, calculate the standard cell potential, and note whether the reaction is spontaneous under standard state conditions.

$Cu (s) │ Cu^{2 +} (a q) ║ Au^{3 +} (a q) │ Au (s)$

Exercises 25

Determine the cell reaction and standard cell potential at 25 °C for a cell made from an anode half-cell containing a cadmium electrode in 1 M cadmium nitrate and a cathode half-cell consisting of an aluminum electrode in 1 M aluminum nitrate solution. Is the reaction spontaneous at standard conditions?

Key terms · 3

standard cell potential $(E_{\text{cell}}^{^\circ})$: the cell potential when all reactants and products are in their standard states (1 bar or 1 atm or gases; 1 M for solutes), usually at 298.15 K
standard hydrogen electrode (SHE): half-cell based on hydrogen ion production, assigned a potential of exactly 0 V under standard state conditions, used as the universal reference for measuring electrode potential
standard electrode potential ($(E_X^{^\circ})$): electrode potential measured under standard conditions (1 bar or 1 atm for gases; 1 M for solutes) usually at 298.15 K

Learn 17.3 on the whiteboard

The tutor teaches the whole section, drawing it out step by step and answering your questions as you go.

Read 17.3 in the textbook · This section on openstax.org