Identify the disproportionation reaction among the following:
1.
2.
3.
4.
Assertion (A): | The decomposition of hydrogen peroxide to form water and oxygen is an example of a disproportionation reaction. |
Reason (R): | The oxygen of peroxide is in –1 oxidation state and it is converted to zero oxidation state in O2 and –2 oxidation state in H2O. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True but (R) is False. |
4. | (A) is False but (R) is True. |
The oxidising agent and reducing agent in the given reaction are
1. Oxidising agent = ; Reducing agent =
2. Oxidising agent = ; Reducing agent =
3. Oxidising agent = ; Reducing agent =
4. None of the above
Given below are two statements:
Assertion (A): | In the reaction between potassium permanganate and potassium iodide, permanganate ions act as an oxidising agent. |
Reason (R): | The oxidation state of manganese changes from +2 to +7 during the reaction. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True but (R) is False. |
4. | (A) is False but (R) is True. |
The set of metals that can show disproportionation reaction is:
1. Cu, Na, Li
2. Mg, F, Ne
3. P, Cl, S
4. Mn, Cu, Ga
The number of moles of MnO-4 required to oxidise one mole of ferrous oxalate completely in an acidic medium is-
1. 0.6 mole
2. 0.4 mole
3. 7.5 moles
4. 0.2 mole