Which statement about standard reduction potentials is correct?

Question

Which statement about standard reduction potentials is correct? (A) E H + / H 2°>0 (B) E D + / D 2°<0 (C) A redox reaction is feasible if sum of SRP of oxidant and that of reductant is a positive quantity. (D) K 2 Cr 2 O 7 is stronger oxidising agent than KMnO 4 in acidic medium.

Tardigrade Admin · Accepted Answer

For a spontaneous reaction, Δ G=- ve which is possible if E° is +ve because, Δ G=-n F E°

Q. Which statement about standard reduction potentials is correct?

$E_{H^{+} / H_{2}}^{\circ} > 0$

$E_{D^{+} / D_{2}}^{\circ} < 0$

A redox reaction is feasible if sum of SRP of oxidant and that of reductant is a positive quantity.

$K_{2} C r_{2} O_{7}$ is stronger oxidising agent than $K M n O_{4}$ in acidic medium.

For a spontaneous reaction, $Δ G = - v e$

which is possible if $E^{\circ}$ is +ve because, $Δ G = - n F E^{\circ}$

Q. Which statement about standard reduction potentials is correct?

EH+/H2​∘​>0

ED+/D2​∘​<0

A redox reaction is feasible if sum of SRP of oxidant and that of reductant is a positive quantity.

K2​Cr2​O7​ is stronger oxidising agent than KMnO4​ in acidic medium.

For a spontaneous reaction, ΔG=−ve which is possible if E∘ is +ve because, ΔG=−nFE∘

$E_{H^{+} / H_{2}}^{\circ} > 0$

$E_{D^{+} / D_{2}}^{\circ} < 0$

$K_{2} C r_{2} O_{7}$ is stronger oxidising agent than $K M n O_{4}$ in acidic medium.

For a spontaneous reaction, $Δ G = - v e$

which is possible if $E^{\circ}$ is +ve because, $Δ G = - n F E^{\circ}$