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Problem: Consider the following reaction below in which pure iron is produced from iron(III) oxide in a blast furnace:          3 CO (g) + Fe2O3 (g) → 2 Fe (l) + 3 CO2 (g)Which reactant is being oxidized and which reactant is being reduced?A. Both CO (g) and Fe2O3 (g) are being reduced.B. Both CO (g) and Fe2O3 (g) are being oxidized.C. CO (g) is being reduced and Fe2O3 (g) is being oxidized.D. CO (g) is being oxidized and Fe2O3 (g) is being reduced.E. Neither CO (g) or Fe2O3 (g) is being oxidized or reduced.

FREE Expert Solution

We’re being asked which of the given reactant is being oxidized and which reactant is being reduced

 Recall the mnemonics LEO GER.

Lose               Gain

Electron         Electrons

Oxidation       Reduction

To be able to identify we first need to see how the oxidation numbers change. 

The rules for oxidation states are as follows:

A. General Rules:

1. For an atom in its elemental form (Zn, Cl2, C(graphite), etc.)    O.S. = 0

2. For an ion (Li+, Al3+, etc.)                                                       O.S. = charge

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Problem Details

Consider the following reaction below in which pure iron is produced from iron(III) oxide in a blast furnace:

          3 CO (g) + Fe2O3 (g) → 2 Fe (l) + 3 CO2 (g)

Which reactant is being oxidized and which reactant is being reduced?

A. Both CO (g) and Fe2O3 (g) are being reduced.
B. Both CO (g) and Fe2O3 (g) are being oxidized.
C. CO (g) is being reduced and Fe2O3 (g) is being oxidized.
D. CO (g) is being oxidized and Fe2O3 (g) is being reduced.
E. Neither CO (g) or Fe2O3 (g) is being oxidized or reduced.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Redox Reactions concept. If you need more Redox Reactions practice, you can also practice Redox Reactions practice problems.