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$H _2( g )+\frac{1}{2} O _2( g ) \rightarrow H _2 O (\ell)$
The work derived from the cell on the consumption of $1.0 \times 10^{-3} mol$ of $H _2( g )$ is used to compress $1.00 mol$ of a monoatomic ideal gas in a thermally insulted container. What is the change in the temperature (in $K$ ) of the ideal gas ?
The standard reduction potentials for the two half-cells are given below.
$\left. O _2( g )+4 H ^{+} \text {(aq. }\right)+4 e ^{-} \rightarrow 2 H _2 O (\ell), E ^{\circ}=1.23 V,$
$\left.2 H ^{+} \text {(aq. }\right)+2 e ^{-} \rightarrow H _2( g ), E ^{\circ}=0.00 V.$
Use $F =96500 C mol ^{-1}, R =8.314 J mol ^{-1} K ^{-1}$
[Given : Density of acetic acid is $1.02\, g\, mL ^{-1}$
Molar mass of acetic acid is $60 \,g\, mol ^{-1}$
$\left.K _{ f }\left( H _{2} O \right)=1.85\, K\, kg\, mol ^{-1}\right]$