A fuel cell involves combustion of the butane at at 1 atm and 298 K
$\underset{(g)}{C_{4} H_{10}} + \underset{(g)}{\frac{13}{2} O_{2}} \to \underset{(g)}{4 C O_{2}} + \underset{(l)}{5 H_{2} O}$
$Δ G ° = - 2746$ kJ/mole
The value of $E_{c e l l}^{o}$ is nearly?

Question

A fuel cell involves combustion of the butane at at 1 atm and 298 K C 4 H 10 ( g ) + 13 2 O 2 ( g ) → 4 C O 2 ( g ) + 5 H 2 O ( l ) Δ G ° = - 2746 kJ/mole The value of E c e l l o is nearly?

TestHub · Accepted Answer

C 4 - 10 H 10 ( g ) + 13 2 O 2 ( g ) → 4 C O 2 + 4 ( g ) + 5 H 2 O ( l ) Here total change in oxidation number of C-atoms = + 16 - ( - 10 ) = + 26 It means total number of e - involved = 26 As E c e l l o - - Δ G ° n F = - ( - 2746 ) × 1000 26 × 96500 = + 1.09 V ≈ 1.0 V

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