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]

Question

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] (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

Δ r G °=- nFE ° =-1 × 96500 × 1.02 =-98430 J =-98.43 kJ

Q. Calculate standard free energy change (in kilojoules) for the reaction,
$\frac{1}{2} C u_{(s)} + \frac{1}{2} C l_{2 (g)} ⇌ \frac{1}{2} C u^{2 +} + C l^{-}$ taking place at $2 5^{\circ} C$ in a cell whose standard e.m.f. is $1.02$ volts. $[1 F = 96500 C m o l^{- 1}]$

$Δ_{r} G^{\circ} = - n F E^{\circ}$
$= - 1 \times 96500 \times 1.02$
$= - 98430 J$
$= - 98.43 k J$

Q. Calculate standard free energy change (in kilojoules) for the reaction, 21​Cu(s)​+21​Cl2(g)​⇌21​Cu2++Cl− taking place at 25∘C in a cell whose standard e.m.f. is 1.02 volts. [1F=96500Cmol−1]

Δr​G∘=−nFE∘ =−1×96500×1.02 =−98430J =−98.43kJ

Q. Calculate standard free energy change (in kilojoules) for the reaction,
$\frac{1}{2} C u_{(s)} + \frac{1}{2} C l_{2 (g)} ⇌ \frac{1}{2} C u^{2 +} + C l^{-}$ taking place at $2 5^{\circ} C$ in a cell whose standard e.m.f. is $1.02$ volts. $[1 F = 96500 C m o l^{- 1}]$

$Δ_{r} G^{\circ} = - n F E^{\circ}$
$= - 1 \times 96500 \times 1.02$
$= - 98430 J$
$= - 98.43 k J$