Standard reduction potentials of the half-reactions are given below:
The strongest oxidizing and reducing agents, respectively, are:
1. and
2. and
3. and
4. and
A solution contains Fe2+, Fe3+ and I– ions. This solution was treated with iodine at 35°C. E° for Fe3+/Fe2+ is +0.77 V and E° for I2/2I– = 0.536 V.
The favourable redox reaction is:
1. Fe2+ will be oxidized to Fe3+.
2. I2 will be reduced to I–.
3. There will be no redox reaction.
4. I– will be oxidized to I2.
The number of moles of KMnO4 that will be needed to react with one mole of sulphite ion in an acidic solution is:
1. | \(3 \over 5\) | 2. | \(4 \over 5\) |
3. | \(2 \over 5\) | 4. | 1 |
Number of moles of \(MnO^-_4\) required to oxidise one mole of ferrous oxalate completely in an acidic medium will be:
1. | 0.6 mole | 2. | 0.4 mole |
3. | 7.5 moles | 4. | 0.2 mole |
The strongest oxidizing agent in the above equation is:
1.
2.
3.
4.
Oxidation numbers of P in , of S in and that of Cr in are respectively:
1. +5, +6 and +6
2. +3, +6 and +5
3. +5, +3 and +6
4. -3, +6 and +6
A mixture of potassium chlorate, oxalic acid and sulphuric acid is heated. During the reaction which element undergoes maximum change in the oxidation number?Redox Reactions
1. S
2. H
3. Cl
4. C
The highest oxidation number of nitrogen among the following compounds is:
1. | 2. | ||
3. | 4. |
The change in oxidation number of chlorine when Cl2 gas reacts with hot and concentrated sodium hydroxide solution is:
1. Zero to +1 and Zero to –5
2. Zero to –1 and Zero to +5
3. Zero to –1 and Zero to +3
4. Zero to +1 and Zero to –3
(a) H2O2 + O3 → H2O + 2O2
(b) H2O2 + Ag2O → 2Ag + H2O + O2
The role of hydrogen peroxide in the above reactions is respectively:
1. | Oxidizing in (a) and reducing in (b) |
2. | Reducing in (a) and oxidizing in (b) |
3. | Reducing in (a) and (b) |
4. | Oxidizing in (a) and (b) |