Calculate E_("cell")^(0) of given electrochemical cell: Zn(s)+Cu^(2+) to Zn^(2+) (aq)+Cu(s) Given : E_(Zn^(2+)//Zn)^(0)=-0.76V E_(Cu^(2+)//Cu)^(0)=0.34V
Calculate E_(cell)^(0) of (at 298K) Zn(s)//ZnSO_(4)(aq)||CuSO_(4)(aq)//Cu(s) given that E_(Zn//Zn^(2+)(aq))^(0)=0.76V E_(Cu(s)//Cu^(2+)(aq))^(0)=-0.34V
Can a solution of 1 M ZnSO_(4) be stored in a vessel made of copper ? Given that E_(Zn^(+2)//Zn)^(@) =-0.76V and E_(Cu^(+2)//Cu)^(@)=0.34 V
Calculate e.m.f. of the cell, Zn//Zn^(2+)(aq) (0.01 M) ||Cd^(2+) (0.1 M)|Cd at 298 K. (Given E_(Zn^(2+)//Zn)^(@)=-0.76 V , E_(Cd^(2+)//Cd=-0.40 V )