Chemistry Oxidation-Reduction help!

Construct a complete balanced oxidation-reduction reaction for each pair of half reactions:

A) H2 -> 2H+ + 2e- and Fe2+ -> Fe3+ + e-

B) 1/4O2(g) + H+ + e- --> 1/2 H2O and H2 --> 2H+ + 2e-

C) 2IO3- + 12H+ + 10e- --> I2 + 6H2O and 2I- = I2 + 2e-


Thanks for your help. If you can show or write each step that would be great!

A. 2e- + 2 Fe+++(aq) ------> 2 Fe++(aq)
....H2(g) -------> 2 e- + 2 H+(aq)
H2(g) + 2 Fe+++(aq) ------------> 2 H+(aq) + 2 Fe++(aq)

B. 1/2 O2(g) + 2 H+(aq) + 2e- ----------> H2O(l)
..........H2(g) ---------> 2 H+(aq) + 2e-
1/2 O2(g) + H2(g) ---------> H2O

C. IO3-(aq) + 6 H+(aq) + 5e- ----------> 1/2 I2(s) + 3 H2O(l)
5 I-(aq) --------> 2.5 I2(s)
IO3-(aq) + 5 I-(aq) + 6 H+(aq) --------> 3 H2O(l) + 3 I2(s)