The method that can be used to find out the strength of the reductant/oxidant in a solution is:

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

What are the values of a, b, c, and d if the chemical reaction below is assumed to be balanced?

$I{O}_3^{-}+a{I}^{-}+b{H}^{+}\to c{H}_{2}O+d{I}_2$

1. 5, 6, 3, 3 

2. 5, 3, 6, 3

3. 3, 5, 3, 6

4. 5, 6, 5, 5