315395 The more positive the value of \(\mathrm{E^{\circ}}\), the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.
\(\mathrm{E^{\Theta}}\) values: \(\mathrm{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}=+0.77 ; I_{2}(s) / I^{-}=+0.54}\);
\(\mathrm{\mathrm{Cu}^{2+} / \mathrm{Cu}=+0.34 ; \mathrm{Ag}^{+} / \mathrm{Ag}=+0.80 \mathrm{~V}}\)

315396 (I) \(\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{O}_{3} \rightarrow \mathrm{H}_{2} \mathrm{O}+2 \mathrm{O}_{2}\)
(II) \(\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{Ag}_{2} \mathrm{O} \rightarrow 2 \mathrm{Ag}+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}\)
Role of hydrogen peroxide in the above reactions is, respectively

315397 Statement A :
A negative value of \(\mathrm{E^{\circ}}\) means that the redox couple is weaker reducing agent than the \(\mathrm{\mathrm{H}^{+} / \mathrm{H}_{2}}\) couple.
Statement B :
A negative \(\mathrm{\mathrm{E}^{\circ}}\) means that the redox couple is stronger reducing agent than the \(\mathrm{\mathrm{H}^{+} / \mathrm{H}_{2}}\).

315398 Standard reduction electrode potentials of three metals A, B and C are \(\mathrm{+0.5 \mathrm{~V},-3.0 \mathrm{~V}}\) and \({\rm{ - 1}}{\rm{.2 }}\) \(\mathrm{\mathrm{V}}\). The reducing powers are in the order

315395 The more positive the value of \(\mathrm{E^{\circ}}\), the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.
\(\mathrm{E^{\Theta}}\) values: \(\mathrm{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}=+0.77 ; I_{2}(s) / I^{-}=+0.54}\);
\(\mathrm{\mathrm{Cu}^{2+} / \mathrm{Cu}=+0.34 ; \mathrm{Ag}^{+} / \mathrm{Ag}=+0.80 \mathrm{~V}}\)

315396 (I) \(\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{O}_{3} \rightarrow \mathrm{H}_{2} \mathrm{O}+2 \mathrm{O}_{2}\)
(II) \(\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{Ag}_{2} \mathrm{O} \rightarrow 2 \mathrm{Ag}+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}\)
Role of hydrogen peroxide in the above reactions is, respectively

315397 Statement A :
A negative value of \(\mathrm{E^{\circ}}\) means that the redox couple is weaker reducing agent than the \(\mathrm{\mathrm{H}^{+} / \mathrm{H}_{2}}\) couple.
Statement B :
A negative \(\mathrm{\mathrm{E}^{\circ}}\) means that the redox couple is stronger reducing agent than the \(\mathrm{\mathrm{H}^{+} / \mathrm{H}_{2}}\).

315398 Standard reduction electrode potentials of three metals A, B and C are \(\mathrm{+0.5 \mathrm{~V},-3.0 \mathrm{~V}}\) and \({\rm{ - 1}}{\rm{.2 }}\) \(\mathrm{\mathrm{V}}\). The reducing powers are in the order

315395 The more positive the value of \(\mathrm{E^{\circ}}\), the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.
\(\mathrm{E^{\Theta}}\) values: \(\mathrm{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}=+0.77 ; I_{2}(s) / I^{-}=+0.54}\);
\(\mathrm{\mathrm{Cu}^{2+} / \mathrm{Cu}=+0.34 ; \mathrm{Ag}^{+} / \mathrm{Ag}=+0.80 \mathrm{~V}}\)

315396 (I) \(\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{O}_{3} \rightarrow \mathrm{H}_{2} \mathrm{O}+2 \mathrm{O}_{2}\)
(II) \(\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{Ag}_{2} \mathrm{O} \rightarrow 2 \mathrm{Ag}+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}\)
Role of hydrogen peroxide in the above reactions is, respectively

315397 Statement A :
A negative value of \(\mathrm{E^{\circ}}\) means that the redox couple is weaker reducing agent than the \(\mathrm{\mathrm{H}^{+} / \mathrm{H}_{2}}\) couple.
Statement B :
A negative \(\mathrm{\mathrm{E}^{\circ}}\) means that the redox couple is stronger reducing agent than the \(\mathrm{\mathrm{H}^{+} / \mathrm{H}_{2}}\).

315398 Standard reduction electrode potentials of three metals A, B and C are \(\mathrm{+0.5 \mathrm{~V},-3.0 \mathrm{~V}}\) and \({\rm{ - 1}}{\rm{.2 }}\) \(\mathrm{\mathrm{V}}\). The reducing powers are in the order

315395 The more positive the value of \(\mathrm{E^{\circ}}\), the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.
\(\mathrm{E^{\Theta}}\) values: \(\mathrm{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}=+0.77 ; I_{2}(s) / I^{-}=+0.54}\);
\(\mathrm{\mathrm{Cu}^{2+} / \mathrm{Cu}=+0.34 ; \mathrm{Ag}^{+} / \mathrm{Ag}=+0.80 \mathrm{~V}}\)

315396 (I) \(\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{O}_{3} \rightarrow \mathrm{H}_{2} \mathrm{O}+2 \mathrm{O}_{2}\)
(II) \(\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{Ag}_{2} \mathrm{O} \rightarrow 2 \mathrm{Ag}+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}\)
Role of hydrogen peroxide in the above reactions is, respectively

315397 Statement A :
A negative value of \(\mathrm{E^{\circ}}\) means that the redox couple is weaker reducing agent than the \(\mathrm{\mathrm{H}^{+} / \mathrm{H}_{2}}\) couple.
Statement B :
A negative \(\mathrm{\mathrm{E}^{\circ}}\) means that the redox couple is stronger reducing agent than the \(\mathrm{\mathrm{H}^{+} / \mathrm{H}_{2}}\).

315398 Standard reduction electrode potentials of three metals A, B and C are \(\mathrm{+0.5 \mathrm{~V},-3.0 \mathrm{~V}}\) and \({\rm{ - 1}}{\rm{.2 }}\) \(\mathrm{\mathrm{V}}\). The reducing powers are in the order