If the standard electrode potential for a cell is $2 V$ at $300 K,$ the equilibrium constant $(K)$ for the reaction.

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

at $300 K$ is approximately:

$(R = 8 J K^{- 1} m o l^{- 1}, F = 96000 C m o l^{- 1})$

Question

If the standard electrode potential for a cell is

2 V

at

300 K,

the equilibrium constant

(K)

for the reaction.

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

at

300 K

is approximately:

(R = 8 J K^{- 1} m o l^{- 1}, F = 96000 C m o l^{- 1})

Aicharya · Accepted Answer

&#8710; G = &#8710; G o + R T l n Q At equilibrium &#8710; G = 0 , &#160; Q = k 0 = &#8710; G o + R T &#160; l n K &#8710; G o = - R T &#160; l n K &#160; &#8756; &#8710; G o = - n F E o So - n F E o = - R T &#160; l n k &#8242; n &#8242; factor for the above cell = 2 So - 2 &#215; 96000 &#215; 2 = - 8 &#215; 300 &#160; l n k l n k = 160 k = e 160

If the standard electrode potential for a cell is 2   V at 300   K , the equilibrium constant K…

Solution

If the standard electrode potential for a cell is 2 &#160; V at 300 &#160; K , the equilibrium constant K…

Solution

If the standard electrode potential for a cell is 2 V at 300 K , the equilibrium constant K…