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Reducing Nature of Alkali Metals

19. Iron powd...

Question

19. Iron powder is added to 1.0M solution of CdCl2 at 298K . The reaction occuring is Cd+² + Fe ----------> Cd + Fe+². If standard potential of a cell producing this reaction is 0.037V, the concentration of Cd+² and Fe+² ions in the above reaction at equilibrium respectively will be

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1.0 M

C d^{2 +}

C d^{2 +}

C d^{2 +} (a q) + F e (s) \to C d (s) + F e^{2 +} (a q); E^{o} = 0.037

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.

298 K

2 {A g}^{+} + C d \to 2 A g + {C d}^{2 +}

(E^{o})

{A g}^{+} / A g

{C d}^{2 +} / C d

0.80 V

- 0.40 V

{C d}^{2 +}

0.1 M

{A g}^{+}

0.2 M

E_{c e l l}^{0}

F e + Z n^{2 +} ⇌ F e^{2 +} + Z n

- 0.32 V

F e^{2 +}

1 M Z n^{2 +}

2 A g^{+} + C d \to 2 A g + C d^{2 +}

A g^{+} \to A g

C d^{2 +} \to C d

0.80 v o l t

- 0.40 v o l t

E^{\circ}

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