A large quantity of cobalt metal was dropped into a solution containing Ag+,Fe3+ and Cu2+, all at unit concentration. If E∘Ag+∣Ag=0.799V,E∘Fe3+,Fe2+∣Pt=0.77V,E∘Cu2+∣Cu =0.34V,E∘Fe3+∣Fe=−0.04 V E∘Cu2+,Cu+∣Pt=0.153V and E∘Co2+∣Co=0.28V, then the solution would contain

Since E∘Fe3+,Fe2+∣Pt,E∘Cu2+∣Cu and E∘Ag+∣Ag are greater than E∘Co2+∣Co,Co metal will be able to reduce Fe3+ to Fe2+, Cu2+and Cu and Ag+to Ag.

A large quantity of cobalt metal was dropped into a solution containing Ag+,Fe3+ and Cu2+, all at unit concentration. If E∘Ag+∣Ag=0.799V,E∘Fe3+,Fe2+∣Pt=0.77V,E∘Cu2+∣Cu =0.34V,E∘Fe3+∣Fe=−0.04 V E∘Cu2+,Cu+∣Pt=0.153V and E∘Co2+∣Co=0.28V, then the solution would contain

Since E∘Fe3+,Fe2+∣Pt,E∘Cu2+∣Cu and E∘Ag+∣Ag are greater than E∘Co2+∣Co,Co metal will be able to reduce Fe3+ to Fe2+, Cu2+and Cu and Ag+to Ag.

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A large quantity of cobalt metal was dropped into a solution containing ${Ag}^{+}, {Fe}^{3 +}$ and ${Cu}^{2 +}$ , all at unit concentration. If
$E^{\circ} ({Ag}^{+} ∣ Ag) = 0.799 V, E^{\circ} ({Fe}^{3 +}, {Fe}^{2 +} ∣ Pt) = 0.77 V, E^{\circ} ({Cu}^{2 +} ∣ Cu) = 0.34 V, E^{\circ} ({Fe}^{3 +} ∣ Fe) = - 0.04 V$
$E^{\circ} ({Cu}^{2 +}, {Cu}^{+} ∣ Pt) = 0.153 V$ and $E^{\circ} ({Co}^{2 +} ∣ Co) = 0.28 V$ , then the solution would contain

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Ag, Fe and Cu

Ag, Fe, and ${Cu}^{+}$

${Fe}^{2 +}, Cu$ and ${Co}^{2 +}$

${Fe}^{2 +}, Cu, Ag$ and ${Co}^{2 +}$

answer is D.

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Detailed Solution

Since $E^{\circ} ({Fe}^{3 +}, {Fe}^{2 +} ∣ Pt), E^{\circ} ({Cu}^{2 +} ∣ Cu)$ and $E^{\circ} ({Ag}^{+} ∣ Ag)$ are greater than $E^{\circ} ({Co}^{2 +} ∣ Co), Co$ metal will be able to reduce ${Fe}^{3 +}$ to ${Fe}^{2 +}, {Cu}^{2 +}$ and $Cu$ and ${Ag}^{+}$ to Ag.