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Worksheet on Redox
1.For the reaction, 2Cr2+ + Cl2(g)  2Cr3+ + 2Cl – , Ecell is 1.78 V. What is Ecell for
the related reaction Cr3+ + Cl –  Cr2+ + 1/2 Cl2(g)
2. What is the oxidation number of Fe in K3Fe(CN)6 ?
3.Which of the following reactions does not represent an oxidation-reduction reaction?
3Al + 6HCl  3H2 + AlCl3
2H2O  2H2 + O2
2NaCl + Pb(NO3)2  PbCl2 + 3NaNO3
2NaI + Br2  2NaBr + I2
4. What element is oxidized in the following reaction?
Cd + NiO2 + 2H2O  Cd(OH)2 + Ni(OH)2
5. Complete and balance the following redox equation. When balanced with whole
number coefficients, the coefficient of S is:
H2S + HNO3  S + NO (acidic solution)
6. Complete and balance the following redox equation. What is the coefficient of H2O
when the equation is balanced with the set of smallest whole numbers?
MnO4– + I –  MnO2 + IO3– (basic solution)
7. The overall reaction: 2Co3+(aq) + 2Cl – (aq)  2Co2+(aq) + Cl2(g)
has the standard cell voltage Ecell= 0.46 V
Given: Cl2(g) + 2e –  2Cl – (aq) E = 1.36 V
Calculate the standard reduction potential for following the half reaction at 25C:
Co3+ + e –  Co2+ E Co3+/Co2+ = ?
8. Pick out the one reaction below that will occur spontaneously.
Mg2+ + Ca  Mg + Ca2+
Au + 3K+  Au3+ + 3K
2Al3+ + 3Fe  2Al + 3Fe2+
Cu + 2H+  Cu2+ + H2
9. Given the following standard reduction potentials in acid solution
E(V)
–1.66
Al3+ + 3e –
Al(s)
+0.07
AgBr(s) + e –
Ag(s) + Br –
+0.14
Sn4+ + 2e –
Sn2+
+0.77
Fe3+ + e –
Fe2+
The strongest oxidizing agent among those shown above is:
10. Using a table of standard electrode potentials decide which of the following
statements is completely true.
Cu2+ can oxidize H2, and Fe can reduce Mn2+.
Ni2+ can oxidize Cu2+, and Fe2+ can reduce H+.
Fe2+ can oxidize H2, and Fe2+ can reduce Au3+.
Br2 can oxidize Ni, and H2 can reduce Mn2+.
H+ can oxidize Fe, and Ni can reduce Br2.