For the following cell, Zn(.s.)|.ZnSO4(.aq.)|.|.CuSO4(.aq.)|.Cu(.s.) when the concentration of Zn2 + is 10 times the concentration of Cu2 + , the expression for Δ G (in J mol- 1 ) is [F is Faraday constant; R is gas constant; T is temperature; E°(cell) = 1.1 V]

Question

For the following cell, Zn(.s.)|.ZnSO4(.aq.)|.|.CuSO4(.aq.)|.Cu(.s.) when the concentration of Zn2 + is 10 times the concentration of Cu2 + , the expression for Δ G (in J mol- 1 ) is [F is Faraday constant; R is gas constant; T is temperature; E°(cell) = 1.1 V] (A) 2.303 RT - 2.2 F (B) - 2.2 F (C) 2.303 RT + 1.1 F (D) 1.1 F

Tardigrade Admin · Accepted Answer

Δ G=Δ G° +2.303RTlog10Q;Q=([. Z n2 + ]./[. C u2 - ].) =-2F(.1.1.)+2.303RTlog1010 =2.303RT-2.2F

Q. For the following cell, Zn(s)∣ZnSO4​(aq)∣∣CuSO4​(aq)∣Cu(s) when the concentration of Zn2+ is 10 times the concentration of Cu2+ , the expression for ΔG (in J mol−1 ) is [F is Faraday constant; R is gas constant; T is temperature; E°(cell) = 1.1 V]

2.303 RT - 2.2 F

- 2.2 F

2.303 RT + 1.1 F

1.1 F

ΔG=ΔG∘+2.303RTlog10​Q;Q=[Cu2−][Zn2+]​ =−2F(1.1)+2.303RTlog10​10 =2.303RT−2.2F

$Δ G = Δ G^{\circ} + 2.303 RTl o g_{10} Q; Q = \frac{[ Z n ^{2 +} ]}{[ C u ^{2 -} ]}$
$= - 2 F (1.1) + 2.303 RTl o g_{10} 10$
$= 2.303 RT - 2.2 F$