In a galvanic cell, reduction occurs at the cathode.

The oxidizing agent is the species that gains electrons and is reduced.

Zinc (Zn) is oxidized to Zn2+.

Ag+ is reduced as it gains electrons to form Ag.

In AgNO3, silver has an oxidation state of +1.

Zinc is oxidized from an oxidation state of 0 to +2.

Cr2O7^2- is reduced to Cr^3+, making it the oxidizing agent.

Carbon (C) is being oxidized to carbon dioxide (CO2).

Fe2O3 is being reduced to Fe as it gains electrons.

Carbon is oxidized as it loses electrons to form CO2.

I^- donates electrons to Fe^3+, thus it is the reducing agent.

Oxygen (O) is oxidized as it goes from 0 in O2 to -2 in H2O.

Hydrogen (H) is oxidized as it goes from an oxidation state of 0 to +1 in NH3.

In Fe2O3, iron has an oxidation state of +3.

Zinc (Zn) is oxidized as it loses electrons to form Zn2+.

In CO2, the oxidation state of carbon is +4.

The oxidation state of carbon changes from -4 in CH4 to +4 in CO2.

In NaClO3, chlorine has an oxidation state of +5.

In NH4+, nitrogen has an oxidation state of -3.

In NO3^-, nitrogen has an oxidation state of +5.

In H2SO4, the oxidation state of sulfur is +6.

The product formed is Fe (iron) when Fe2O3 is reduced by carbon monoxide.

C2O4^2- is the reducing agent as it donates electrons.

Zinc (Zn) is the reducing agent as it donates electrons to copper.

The correct reduction half-reaction in acidic medium is MnO4- + 8H+ + 5e- → Mn2+ + 4H2O.

The correct reduction half-reaction shows the gain of electrons and protons.

The reduction half-reaction is Cu^2+ + 2e^- → Cu.

In acidic medium, MnO4- is reduced to Mn2+.

A catalyst speeds up the reaction without being consumed in the process.

Sodium (Na) can act as a reducing agent as it readily donates electrons.