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).

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Solution

(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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Similar questions

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

(i) $M g (s) | M g^{2 +} (0.001 M) | | C u^{2 +} (0.001 M) | C u (s)$

(ii) $F e (s) | F e^{2 +} (0.001 M) | | H^{+} (1 M) | H_{2} (g) (1 b a r) | P t (s)$

(iii) $S n (s) | S n^{2 +} (0.050 M) | | H^{+} (0.020 M) | H_{2} (g) (1 b a r) | P t (s)$

(iv) $P t (s) | B r_{2} (l) | B r^{-} (0.010 M) | | H^{+} (0.030 M) | H_{2} (g) (1 b a r | P t (s))$

$E_{(\frac{M g^{2 +}}{M g})}^{\circ} = - 2.37 V; E_{(\frac{C u^{2 +}}{C u})}^{\circ} = + 0.34 V; E_{(\frac{F e^{2 +}}{F e})}^{\circ} = - 0.44 V; E_{(\frac{S n^{2 +}}{S n})}^{\circ} = - 0.14 V; E_{(\frac{\frac{1}{B r_{2}}}{B r^{-}})}^{\circ} = + 1.08 V,$