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write the nernst equation and emf of the following...

Question:
Write the Nernst equation and emf of the following cells at 298 K:

(i) Mg(s) | Mg²⁺(0.001M) || Cu²⁺(0.0001 M) | Cu(s)

(ii) Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s)

(iii) Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s)

(iv) Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).

Answer:

(i) For the given reaction, the Nernst equation can be given as:

= 2.7 - 0.02955 = 2.67 V (approximately)

(ii) For the given reaction, the Nernst equation can be given as:

= 0.52865 V = 0.53 V (approximately)

(iii) For the given reaction, the Nernst equation can be given as:

= 0.14 - 0.0295 × log125

= 0.14 - 0.062

= 0.078 V

= 0.08 V (approximately)

(iv) For the given reaction, the Nernst equation can be given as:

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