Redox Reactions...

Analyze the diagram. The left beaker represents the start of the reaction and the right beaker represents the end of the reaction.
Classify this reaction.

The oxidation number of chromium in $$K_{2}CrO_{4}$$ is:

The half-cell reaction is the one that:

What is the number of coulombs required for the conversion of one mole of $$MnO_{4}^{-}$$ to one mole of $$Mn^{2+}$$?

In alkaline medium, the reaction of hydrogen peroxide with potassium permanganate produces a compound in which the oxidation state of $$Mn$$ is:

The oxidation number of chromium in $$\displaystyle Cr{ O }_{ 5 }$$ is:

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half-cell reactions and their standard potentials are given below:
$$Mn{O}_{4}^{-} (aq.) + 8H^{+}(aq.) + 5e^{-} \rightarrow Mn^{2+}(aq.) + 4H_{2}O(l); E^{\circ} = 1.51\ volt$$
$$Cr_{2}O_{7}^{2-}(aq.) + 14H^{+}(aq.) + 6e^{-} \rightarrow 2Cr^{3+}(aq.) + 7H_{2}O(l)' E^{\circ} = 1.38\ volt$$
$$Fe^{3+}(aq.) + e^{-}\rightarrow Fe^{2+}(aq.); E^{\circ} = 0.77\ volt$$
$$Cl_{2}(g) + 2e^{-} \rightarrow 2Cl^{-}(aq.); E^{\circ} = 1.40\ volt$$
Identity the only incorrect statement regarding the quantitative estimation of aqueous $$Fe(NO_{3})_{2}$$.

Oxidation number of nitrogen in which among the oxides of nitrogen is the lowest?

Arrange the following in the increasing order of oxidation state of $$Mn.$$
(i) $$Mn^{2+}$$
(ii) $$MnO_2$$
(iii) $$KMnO_4$$
(iv) $$K_2MnO_4$$.

Oxidation state of $$S$$ in $${SO_4}^{2-}$$ is: