Question

For the reduction of silver ions with copper metal, the standard cell potential is 0.46 V at 25∘C. The value of standard Gibbs energy ΔG∘ will be ​

Answer 1

Answer :

• Standard gibbs energy, ΔG° = -89.0 kJ.

Step-by-step explanation:

Given that,

• Standard cell potential, $\rm{E^{\circ}_{cell}}$ = 0.46 V.
• Temperature, T = 25°C.

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According to the question, cell reaction will be:-

$\rm{2Ag^++Cu\longrightarrow{}Cu^{2+}+2Ag}$

Therefore, n = 2

Also, we know,

Standard Gibbs energy, ΔG° = $\rm{-nFE^{\circ}_{cell}}$

Putting the values, we get,

$:\implies\rm{{\Delta}G^{\circ}=-2\times{}96500\times{}0.46}$

$:\implies\rm{{\Delta}G^{\circ}=-88780\:J}$

$:\implies\rm{{\Delta}G^{\circ}=}\:\bold{-89.0\:kJ\:(approx.).}$

Answer 2

Explanation:

Given E

cell

o

=0.46 V, T=298 K

2Ag

+

+Cu→Cu

2+

+2Ag

n=2

ΔG

o

=−nFE

cell

o

=−2×96500×0.46 V

ΔG=−88780 J/mole

ΔG=−88.78 KJ/mol

ΔG=−89 KJ/mol