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In each of the following balanced oxidation-reduction equations, identify those elements that undergo changes in oxidation...

In each of the following balanced oxidation-reduction equations, identify those elements that undergo changes in oxidation number and indicate the magnitude of the change in each case.


2MnO4−(aq)+3S2−(aq)+4H2O(l)→3S(s)+2MnO2(s)+8OH−(aq)   

4H2O2(aq)+Cl2O7(g)+2OH−(aq)→2ClO2−(aq)+5H2O(l)+4O2(g)

Ba2+(aq)+2OH−(aq)+H2O2(aq)+2ClO2(aq)→Ba(ClO2)2(s)+2H2O(l)+O2(g)

Solutions

Expert Solution

1)

Mn(+7)O(-2)4- + S(-2)2- + H(+1)2O(-2)                      S(0) + Mn(+4)O(-2)2 + O(-2)H(+1)-

Oxidation

S(-2)2-                             S(0)

Thus, oxidation state of Sulphur changes from -2 to 0 (Magnitude of change = 2)

Reduction

Mn(+7)O4-                     Mn(+4)O2

Oxidation state of Manganese changes from +7 to +4 (Magnitude of change = 3)

2)

H(+1)2O(-1)2 + Cl(+7)2O(-2)7 + O(-2)H(+1)-                 Cl(+3)O(-2)2- + H(+1)2O(-2) + O(0)2

Oxidation

H2O(-1)2                       O(0)2

Thus, oxidation state of Oxygen changes from -1 to 0 (Magnitude of change = 1)

Reduction

Cl(+7)2O7                   Cl(+3)O2-

Oxidation state of Chlorine changes from +7 to +3 (Magnitude of change = 4)

3)

Ba(+2)2+ + O(-2)H(+1)- + H(+1)2O(-1)2 + Cl(+4)O(-2)2              Ba(+2)(Cl(+3)O(-2)2)2 + H(+1)2O(-2) + O(0)2

Oxidation

H2O(-1)2                        O(0)2

Thus, oxidation state of Oxygen changes from -1 to 0 (Magnitude of change = 1)

Reduction

Cl(+4)O2                        Ba(Cl(+3)O2)2

Oxidation state of Chlorine changes from +4 to +3 (Magnitude of change = 1)

queen_honey_blossom answered 5 months ago
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