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Calculate the equilibrium constant for the reaction at 298K.
`Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s)`
Given, `E_(Zn^(2+)//Zn)^(@) =- 0.76V` and `E_(Cu^(2+)//Cu)^(@) = +0.34 V`

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Calculate the equilibrium constant for the reaction at 298 K Zn(s)+Cu^(2+)(aq)harr Zn^(2+)(aq)+Cu(s) Given " " E_(Zn^(2+)//Zn)^(@)=-0.76 V and E_(Cu^(2+)//Cu)^(@)=+0.34 V

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(a) Calculate Delta G^@ for the reaction Zn (s) + Cu^(2+) (aq) rarr Zn^(2+) + Cu(s) Given: E^@ for (Zn^(2+))//Zn = -0.76 V and E^@ for (Cu^(2+))//Cu = +0.34 V R= 8.314 JK^-1 mol^(-1) F= 96500 Cmol^(-1) (b) give two advantages of fuel cells.

Calculate the maximum work that can be obtained from the daniell call given below, Zn(s)|Zn^(2+)(aq)||Cu^(2+)(aq)|Cu(s) . Given that E_(Zn^(2+)//Zn)^(@)=-0.76V and E_(Cu^(2+)//Cu)^(@)=+0.34V .

Find the equilibrium constant at 298K for the reaction, Cu^(2+)(aq) +In^(2+)(aq)hArr Cu^(+)(aq) +In^(3+)(aq) Given that E_(Cu^(2+)//Cu^(+))^(@) =0.15V, E_(In^(3+)//In^(-))^(@) =- 0.42V, E_(In^(2+)//In^(+))^(@) =- 0.40V

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