1. Tardigrade
  2. Question
  3. Chemistry
  4. Calculate standard free energy change (in kilojoules) for the reaction, (1/2) Cu ( s )+(1/2) Cl 2( g ) leftharpoons (1/2) Cu 2++ Cl - taking place at 25° C in a cell whose standard e.m.f. is 1.02 volts. [1 F =96500 C mol -1]

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Q. Calculate standard free energy change (in kilojoules) for the reaction,
$\frac{1}{2} Cu _{( s )}+\frac{1}{2} Cl _{2( g )} \rightleftharpoons \frac{1}{2} Cu ^{2+}+ Cl ^{-}$ taking place at $25^{\circ} C$ in a cell whose standard e.m.f. is $1.02$ volts. $\left[1 F =96500\, C\, mol ^{-1}\right]$

Electrochemistry

Solution:

$\Delta_{ r } G ^{\circ}=- nFE ^{\circ}$
$=-1 \times 96500 \times 1.02$
$=-98430\, J$
$=-98.43\, kJ$