Given that: 

 \(\begin{aligned} &E_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{\Theta}=+1.23 \mathrm{~V} ; E_{S_{2} \mathrm{O}_{8}^{2-} / \mathrm{{SO}_{4}}^{-2}}=2.05 \mathrm{~V} \\ &E_{\mathrm{Br}_{2} / \mathrm{Br}^{-}}^{\Theta}=+1.09 \mathrm{~V} ; E_{A u^{3+} / A u}^{\Theta}=+1.4 \mathrm{~V} \end{aligned}\)

Which of the following is the strongest oxidizing agent?
1. \(\mathrm{S}_2 \mathrm{O}_8^{2-}\) ${}_{}$

2. \(\mathrm{O}_2\) ${}_{}$

3. \(A u^{3+}\)$$

4. \(B r_2\)

Which of the following is the strongest reducing agent?

[Given: \(E_{Cl_{2}/Cl^{-}}^{o} = 1.36 V\); \(E_{Cr^{3+}/Cr}^{o} = -0.74 V\); 
\(E_{Cr_20_7^{2-}/Cr^{3+}}^{o} = 1.33 V\) and \(E_{MnO_4^{-}/Mn^{2+}}^{o} = 1.51 V\)]

Standard  reduction electrode potentials of three metals A, B and C are +0.5V , -3.0 V and -1.2 V respectively. The reducing power of these metals are:

Which of the following processes is happening at the anode (from the options given below)?

1. \(\mathrm{F}_2+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{~F}^{-}\)
2. \( \mathrm{H}^{+}+\frac{1}{2} \mathrm{O}_2+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_2 \mathrm{O}\) 
3. \(2Cr^{3+}+7H_2O \rightarrow Cr_2O^{2-}_7 +14H^+ + 6e^-\)
4. None of the above