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Problem: All of the following are oxidation-reduction reactions EXCEPTa. MgCO3(s) → MgO(s) + CO2(g)b. 2 Li(s) + Br2(g) → 2 LiBr(g)c. Fe(s) + 2 HCl(aq) → FeCl2(aq) + H2(g)d. 2 C(s) + O2(g) → 2 CO(g)e. 2 H2O(l) → 2 H2(g) + O2(g)

FREE Expert Solution

We’re being asked which of the given reactions is not a redox reaction. The weakest reducing agent is the strongest oxidizing agent. Oxidizing agents are the species that are being reduced in a redox reaction. Recall the mnemonics LEO GER.

Lose               Gain

Electron         Electrons

Oxidation       Reduction

A change in charge or oxidation state indicates the loss or gain of an electron.

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

B. Specific Rules:

1. Group 1A              O.S. = +1

2. Group 2A              O.S. = +2

3. Hydrogen              O.S. = +1, with nonmetals

                                  O.S. = –1 with metals and boron

4. Fluorine                 O.S. = –1

5. Oxygen                  O.S. = –1 in peroxides (X2O2, X = Group 1A)

                                  O.S. = –1/2 in superoxides (XO2, X = Group 1A)

                                  O.S. = –2 in other compounds

6. Group 7A               O.S. = –1 (except when bonded to O)

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Problem Details

All of the following are oxidation-reduction reactions EXCEPT

a. MgCO3(s) → MgO(s) + CO2(g)

b. 2 Li(s) + Br2(g) → 2 LiBr(g)

c. Fe(s) + 2 HCl(aq) → FeCl2(aq) + H2(g)

d. 2 C(s) + O2(g) → 2 CO(g)

e. 2 H2O(l) → 2 H2(g) + O2(g)

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