Mg(s) + Fe²+ (aq) →→ Mg²+ (aq) + Fe(s) The galvanic cell described above has a standard cell potential of 1.93 V. The standard reduction potential of Mg2+ corresponding to the half-reaction Mg2+ (aq) + 2e- Mg(s) is -2.37 V. Calculate the standard reduction potential of iron(II). EFe²+ -1.4

Mg(s) + Fe²+ (aq) →→ Mg²+ (aq) + Fe(s) The galvanic cell described above has a standard cell potential of 1.93 V. The standard reduction potential of Mg2+ corresponding to the half-reaction Mg2+ (aq) + 2e- Mg(s) is -2.37 V. Calculate the standard reduction potential of iron(II). EFe²+ -1.4

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ISBN:9781305957404

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Chapter1: Chemical Foundations

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

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X Incorrect.
Mg(s) + Fe²+ (aq) → Mg²+ (aq) + Fe(s)
The galvanic cell described above has a standard cell potential of 1.93 V. The standard reduction potential of Mg2+ corresponding to
the half-reaction
Mg2+ (aq) + 2e- Mg(s) is -2.37 V.
Calculate the standard reduction potential of iron(II).
EFe²+
= -1.4
V

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