Your laboratory instructor will assign a number of the following redox equations

Question

Your laboratory instructor will assign a number of the following redox equations to balance. Balance them on your own paper and submit them at tne designated ime. Show the balanced oxidation and reduction half-reactions, underline the reducing 2 gent, and the oxidizing agent in the final balanced equaion. lution) (acidie solution) 4. Hgs) NOs ag)- C (ag)-HgCLa () NOG) -S(a) (acidic solution) lution) (acidic solution) 7. Woxe) Sn2 (aq) .Claa)-Woss) SnCls2 (Caq) (acidic solution) ution) (acidic solution) (acidic solution) acidic solution) (acidic solution) (acidic solution) 11. Tco4(aa) TIG) -Te(ag) 13. CHutg) Mnoag) -Mn2 (ag)+ co2() (acidic solution utiop) 16. Bi(OH)3(s) SnO2 (ag)-Bi(s)+SnOs (aq) 17. Mnos2 (aq) - Mn04'(aa)+Mn02(s) (basic soiution) tasic solution (basic solution (basic solution)

Explanation / Answer

Solved the first four parts, post multiple question to get the remaining answers

1)

Oxidation Half

H2S(g) ------- > S(g) + 2H+ + 2e-

Reduction Half

NO3- (aq) + 4H+ + 3e- ------- NO(g) + 2H2O

Multiply the first reaction by 3 and second by 2 to cancel the e- we get

2NO3- (aq) + 3H2S + 2H+ ------- 2NO(g) + 4H2O + 3S(s)

2)

Oxidation Half

2Cl-(aq) ------ > Cl2(g) + 2e-

Reduction Half

MnO4-(aq) -+ 8H+ + 5e- ------- Mn(2+)(aq) + 4H2O

Multiply first reaction by 5 and second by 2 to cancel the electrons we get

10Cl- + 2MnO4- + 16H+ ---------- 2Mn(2+) + 8H2O + 5Cl2(g)

5)

Oxidation Half

Fe(2+) (aq) ------ > Fe(+3)(aq) + e-

Reduction Half

MnO4-(aq) -+ 8H+ + 5e- ------- Mn(2+)(aq) + 4H2O

Multiply first reaction by 5 and second by 1 to cancel the electrons we get

5Fe(2+) + MnO4- + 8H+ ---------- 5Fe(3+) + 4H2O + Mn(2+)(aq)

8)

Oxidation Half

Ag(s) ------ > Ag+(aq) + e-

Reduction Half

NiO2(s) + 4H+ + 2e- --------> Ni(2+)(aq) + 2H2O

Multiply first reaction by 2 and second by 1 to cancel the electrons we get

2Ag(s) + NiO2(s) + 4H+ ---------- Ni(2+) + 2Ag+(aq) + 2H2O

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