Classical Idea of Redox Reactions

The standard reduction potentials at 298 K for the following half reactions are given against each:
$\begin{array}{l}{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{e}\stackrel{}{\rightleftharpoons }\mathrm{Zn}\left(\mathrm{s}\right) ;-0.762\\ {\mathrm{Cr}}^{3+}\left(\mathrm{aq}\right)+3\mathrm{e}\stackrel{}{\rightleftharpoons }\mathrm{Cr}\left(\mathrm{s}\right) ; -0.740\\ 2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+2\mathrm{e}\stackrel{}{\rightleftharpoons }{\mathrm{H}}_2\left(\mathrm{g}\right) ; 0.000\\ {\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+\mathrm{e}\stackrel{}{\rightleftharpoons }{\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right) ; 0.770\end{array}$
Which is the strongest reducing agent?

Which of the following reactions is possible at the anode?

Which is reduced in the following reaction

$\left(\mathrm{a}\right)2\mathrm{KI}\left(\mathrm{aq}\right)+\left(\mathrm{b}\right){\mathrm{Cl}}_2\left(\mathrm{aq}\right)\to 2\mathrm{KCl}+{\mathrm{I}}_2\left(\mathrm{aq}\right)$

What happens to the solution of ferric chloride acidified with $\mathrm{HCl}$, when hydrogen is bubbled through it?

A solution of ferric chloride acidified with $\mathrm{HCl}$ is unaffected when hydrogen is bubbled through it, but gets reduced when $\mathrm{Zn}$ is added to same acidified solution. Why?

What will be the main product in the reaction happens between potassium ferrocyanide and hydrogen peroxide?

Which of the following will be the equation for the reaction happens between potassium ferrocyanide and hydrogen peroxide?

Define redox reactions based on the electropositive part? 

Which compound among the following can act as both an oxidizing and a reducing agent ?

Discuss how does the reduction reaction involved in alkenes.

Express the definition of reduction based on the classical concept.

Define reduction based on the classical concept.

The addition of the electropositive element is known as 

Define reduction in classical way.

Hydrogen gas acts as a

${\mathrm{Zn}}_{\left(\mathrm{s}\right)} + {{\mathrm{CuSO}}_4}_{\left(\mathrm{aq}\right)} \to {{\mathrm{ZnSO}}_4}_{\left(\mathrm{aq}\right)} + {\mathrm{Cu}}_{\left(\mathrm{s}\right)}$

Above reaction is an example of:

${\mathrm{Zn}}_{\left(\mathrm{s}\right)} + {{\mathrm{CuSO}}_4}_{\left(\mathrm{aq}\right)} \to {{\mathrm{ZnSO}}_4}_{\left(\mathrm{aq}\right)} + {\mathrm{Cu}}_{\left(\mathrm{s}\right)}$

Above reaction is an example of:

In which of the following reactions does the underlined species get oxidised?

Which of the following is not a redox reaction?