The rusting of iron takes place as follows:
$2 H^{\oplus} + 2 e^{-} + \frac{1}{2} O_{2} \to H_{2} O (l); E^{⊖} = + 1.23 V$
$F e^{2 +} (a q) + 2 e^{-} \to F e (s); E^{⊖} = - 0.44 V$
Calculate $Δ G^{⊖}$ for the net process.

Question

The rusting of iron takes place as follows:

2 H^{\oplus} + 2 e^{-} + \frac{1}{2} O_{2} \to H_{2} O (l); E^{⊖} = + 1.23 V

F e^{2 +} (a q) + 2 e^{-} \to F e (s); E^{⊖} = - 0.44 V

Calculate

Δ G^{⊖}

for the net process.

Toppr Admin · Accepted Answer

E-x2296-cell-1-23-x2212-x2212-0-44-1-67V-x21D2-x394-G-x2296-cell-nFE-x2296-cell-x2212-2-xD7-96500-xD7-1-67Jmol-x2212-1-x2212-332-3kJmol-x2212-1

The rusting of iron takes place as follows : $2 H^{+} + 2 e + \frac{1}{2} O_{2} \to H_{2} O (l); E^{o} = + 1.23 V$
$F e^{2 +} + 2 e \to F e (s); E^{o} = - 0.44 V$
$Δ G^{o}$ for the net process is:
$- 322$ $k J m o l^{- 1}$
$- 76$ $k J m o l^{- 1}$
$- 161$ $k J m o l^{- 1}$
$- 152$ $k J m o l^{- 1}$