The standard Gibbs energy for the given cell reaction in $k J m o l^{- 1}$ at $298 K$ is:
$Z n (s) + C u^{2 +} (a q) ⟶ Z n^{2 +} (a q) + C u (s)$ ,
$E^{0} = 2 V a t 298 K$
$(F a r a d a y' s c o n s t a n t, F = 96000 C m o l^{- 1})$

Question

The standard Gibbs energy for the given cell reaction in

k J m o l^{- 1}

at

298 K

is:

Z n (s) + C u^{2 +} (a q) ⟶ Z n^{2 +} (a q) + C u (s)

,

E^{0} = 2 V a t 298 K

(F a r a d a y' s c o n s t a n t, F = 96000 C m o l^{- 1})

Aicharya · Accepted Answer

For the reaction, C u 2 + a q + Z n s &#10230; Z n 2 + a q + C u s n = 2 , two electrons are exchanged &#8710; G o = - n F E o = - 2 &#215; 96000 &#215; 2 = - 384000 = - 384 &#160; k J

The standard Gibbs energy for the given cell reaction in k J   m o l - 1 at 298   K is: Z n s + C…

Solution

The standard Gibbs energy for the given cell reaction in k J &#160; m o l - 1 at 298 &#160; K is: Z n s + C…

Solution

The standard Gibbs energy for the given cell reaction in k J m o l - 1 at 298 K is: Z n s + C…