Calculate the standard cell potentials of galvanic cell in which the following reactions take place-i 2Crs - 3Cd2-aq - 2Cr3-aq - 3Cdii Fe2-aq - Ag- aq - Fe3-aq - AgsCalculate the -rG- and equilibrium constant of the reactions

(i) E^o_cell = E^0_cathode E^0_anode = 0.40 ( 0.74) = 0.34 V Δ G^0 = nFE^o_cell = 6 × 96500 × 0.34 = 196860 J/mol = 196.86 kJ/mol #160; ...

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Equilibrium Constant and Standard Free Energy Change

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Question

Calculate the standard cell potentials of galvanic cell in which the following reactions take place:
(i) $2 C r (s) + 3 C d^{2 +} (a q) \to 2 C r^{3 +} (a q) + 3 C d$
(ii) $F e^{2 +} (a q) + A g^{+} (a q) \to F e^{3 +} (a q) + A g (s)$
Calculate the $Δ_{r} G^{⊖}$ and equilibrium constant of the reactions

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Calculate the standard cell potentials of galvanic cells in which the following reactions take place:

(i) 2Cr(s) + 3Cd²⁺(aq) → 2Cr³⁺(aq) + 3Cd

(ii) Fe²⁺(aq) + Ag⁺(aq) → Fe³⁺(aq) + Ag(s)

Calculate the Δ_rG^θ and equilibrium constant of the reactions.

Calculate the standard cell potentials of galvanic cell in which the following reactions take place :

(i) $2 C r (s) + 3 C d^{2 +} (a q) \to 2 C r^{3 +} (a q) + 3 C d$

(ii) $F e^{2 +} (a q) + A g^{+} (a q) \to F e^{3 +} (a q) + A g (s)$

Calculate the $Δ_{r} G^{\circ}$ and equilibrium constant for the reactions

2 C r_{(s)} + 3 C d_{(a q)}^{2 +} \to 2 C r_{(a q)}^{3 +} + 3 C d_{(s)}

E_{C r^{3 +} / C r}^{o} = - 0.74

E_{C d^{2 +} / C d}^{o} = - 0.40

3.1

F e^{3 +} (a q)

I^{-} (a q)

A g^{+} (a q)

C u (s)

F e^{3 +} (a q)

B r^{-} (a q)

A g (s)

F e^{3 +} (a q)

B r_{2} (a q)

F e^{2 +} (a q)

E^{o}

2 A g^{+} (a q) + S n^{2 +} (a q) \to S n^{4 +} (a q) + 2 A g (s)

A g (s) + \frac{1}{2} S n^{4 +} (a q) \to \frac{1}{2} S n^{2 +} (a q) + A g^{+} (a q)

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