1.

For the reaction H_2(g)+2AgCl(s)=2Ag(s)+2H^+ (aq)(0.1M)+2Cl^(-) (aq)(0.1M) (1 atm) Delta G^@=42927 joules at 25^@C.Calculate the emf of the cell in which the given reaction takes place .

Answer»

SOLUTION :We know
`DELTAG^@=-NFE^@`
`therefore E^@=- (DeltaG^@)/(nF)=42927/(2 times 96500)=0.2224` volt
Now, for the above cell REACTION
`E_(cell),E^@-0.0591/2log""([H^+]^2[Cl^-]^2)/([H_2])`
`=0.2224-0.0591/2log""((0.1)^2(0.1)^2)/((1))`
`=0.3406` volt
`therefore E_(Hg_2^(2+))^@=0.77+00.021=0.791` volt


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