Given below are a set of half-cell reactions (in acidic medium) alongwith their E° (in volt) values.
l2+2e- → 2l- |
E°= 0.54 |
Cl2+2e- → 2Cl- |
E°= 1.3 |
Mn+3 +e- →Mn+2 |
E°= 1.50 |
Fe+3+e- → Fe+2 |
E°= 0.7 |
O2+4H+4e →2H2O |
E°= 1.23 |
1.Among the following, identify the correct statement
(1) Cl– is oxidised by O2
(2) Fe+2 is oxidised by iodine
(3) I– is oxidised by chlorine
(4) Mn+2 is oxidised by chlorine
2. While Fe+3 is stable, Mn+3 is not stable in acid solution because
(1) O2 oxidises Mn+2 to Mn+3
(2) O2 oxidises both Mn+2 to Mn+3 and Fe+2 to Fe+3
(3) Fe+3 oxidises H2O to O2
(4) Mn+3 oxidises H2O to O2
3.The strongest reducing agent in aqueous solution is
(1) I– (2) Cl– (3) Mn+2 (4) Fe+2