Chemistry, asked by manz, 1 year ago

for the reaction to AgCl + H2 gives to 2Ag + 2H^+ (.1 M) + 2 CL^- (1.1 molar) if Delta G° is equal to -43600j at 25 degree Celsius calculate the EMF of the cell

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Answered by kobenhavn
21

Answer:  The EMF of the cell is 0.165 V.

Explanation: The standard emf of a cell is related to Gibbs free energy by following relation:

\DeltaG=-nFE^0

\DeltaG = gibbs free energy

n= no of electrons gained or lost  = 2F= faraday's constant = 96500 C

AgCl+H_2\rightarrow 2Ag+2H^+ (.1 M)+2Cl^-(1.1 M)

-43600=-2\times 96500\times E^0

E^0=0.225V

Using Nernst equation at 25 degree Celsius :

E_{cell}=E^o_{cell}-\frac{0.0592}{n}\log \frac{[H^+]^2}{[Cl^-]^2}

where,

n = number of electrons in oxidation-reduction reaction = 2

E^o_{cell} = standard electrode potential = 0.225V

E_{cell}=.225-\frac{0.0592}{2}\log \frac{[0.1]^2}{[1.1]^2}

E_{cell}=0.165V

Answered by himanshupassey26
2

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