If `K_c` for the reaction `Cu^(2+)(aq)+Sn^(2+)(aq)toSn^(4+)(aq)+Cu(s)` at `25^(@)` C is represented as `2.6xx10^y` then find the value of y. (Given:`E_(Cu^(2+)"|"Cu)^(@)=0.34V,E_(Sn^(4+)"|"Sn^(2+)^(@)=0.15V)`
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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
Sn(s) | Sn^(2+)(aq) || Cu^(2+)(aq) | Cu(s) For the voltaic cell represented above, which change will increase the voltages?
Calculate the value of equilibrium constant for the reaction taking place between Cu(II) and Sn (II) ions in aqueous solution at 298 K. Given : E_(cu^(2+)//cu)^(@)=0.34" V" , E_(Sn^(2+)//Sn^(4+))^(@)=-0.154" V" .
Cu^(2+)(aq.) is unstable in solution and under goes simultaneous oxidation and reduction according to the reaction 2Cu^(+)(aq.)hArr Cu^(2+)(aq.)+Cu(s) Choose the correct E^(@) for the above reaction if E_(Cu^(2+))^(@)//Cu = 0.34 V and E_(Cu^(2+))^(@)//Cu^(+) = 0.15 V