Which of the following is the most powerful oxidizing agent?

1. ${\mathrm{F}}_2$

2. ${\mathrm{Cl}}_2$

3. ${\mathrm{Br}}_2$

4. ${\mathrm{I}}_2$

For the redox reaction, 
${\mathrm{MnO}}_4^{-}+{\mathrm{C}}_2{\mathrm{O}}_4^{2-}+{\mathrm{H}}^{+}\to {\mathrm{Mn}}^{2+}+{\mathrm{CO}}_2+{\mathrm{H}}_2\mathrm{O}$, the correct coefficients of the reactants  ${\mathrm{MnO}}_4^{-},{\mathrm{C}}_2{\mathrm{O}}_4^{-},{\mathrm{H}}^{+}$ for the balanced reaction are, respectively:

1. 2, 5, 16

2. 16, 3, 12

3. 15, 16, 12

4. 2, 16, 5

The oxidation states of phosphorous in H₃PO₃, P₄  and PH₃ respectively are:

1. +3, zero and -3

2. -3, zero and +3

3. +3, +4 and -3

4. +3, zero and +3

Consider the following redox reaction:

3Br₂ + 6CO₃²⁻ + H₂O → 5Br⁻ + BrO₃⁻ + 6HCO₃⁻

Find the correct statement regarding the oxidation and reduction processes in the above reaction.

1. $\mathrm{Br₂\; is\; oxidised\; and\; CO₃²⁻\; is\; reduced.}$

2. Br₂ is reduced and CO₃²⁻ is oxidised.

3. Bromine is both reduced and oxidised.

4. Bromine is neither reduced nor oxidised.

What is the value of $$\(E_{\text {cell }}^o\) for the following reaction?

H₂O₂(aq) + 2H⁺(aq) + 2Fe²⁺ (aq) → 2H₂O(I) + 2Fe³⁺(aq) 

Given that:
\(E_{\mathrm{H}_2 \mathrm{O}_2 / \mathrm{H}_2 \mathrm{O}(1)}^0=+1.763 \mathrm{~V}\)
\(E_{\mathrm{Fe}^{3+}(a q) / \mathrm{Fe}^{2+}(a q)}^0=+0.769 \mathrm{~V}\)

1. 0.225 V

2. 0.994 V

3. 2.532 V

4. 3.301 V

The oxidation number of phosphorus in Mg₂P₂O₇ is:

1. +3

2. +2

3. +5

4. -3

Which of the following is not an oxidation-reduction reaction?

Find the average oxidation state of sulphur in Na₂S₂O₃.

1. -2

2. +2

3. +4

4. +6

Among the following compounds, which one is a transition metal with an oxidation number of zero?

Which of the following is the strongest oxidising agent?

1. $Br{O}_3^{-}/B{r}^{2+},E^o=+1.50$

2. $F{e}^{3+}/F{e}^{2+},E^o=+0.76$

3. $Mn{O}_4^{-}/M{n}^{2+},E^o=+1.52$

4. $C{r}_2{O}_7^{2-}/C{r}^{3+},E^o=+1.33$