Represent the cell and calculate the Standard e.m.f. of the cell having following cell reaction: `2Cr(s)+3Cd^(2+)(aq)to 2Cr^(3+)(aq) + 3 Cd(s) E^0 Cr^(3+)//Cr=-0.73 volt` and `E^0 Cd^(2+)//Cd=-0.40` volt

Calculate the standard emf of the cell having the cell reaction. Zn(s) + Co^(2+) ( aq) rarr Zn^(2+) ( aq) + Co(s) E_(Zn//Zn^(2+)) ^(@) = 0.76V, E_(Co//Co^(2+))^(@) = 0.25V

Calculate the standard cell potential of a galvanic cell in which the following reaction takes place 2Cr(s) + 3Cd^(2+) ( aq) rarr 2Cr^(3+) ( aq) + 3Cd(s) Calculate Delta_( r) G^(@) and equilibrium constant K of the above reaction at 25^(@)C . [Given, E_(Cr^(3+) //Cr)^(@) = - 0.74 V, E_(Cd^(2+)//Cd)^(@) = - 0.40V, 1F = 96500 C "mol"^(-1)]

Calculate the equilibrium constant for the reaction. Fe(s) + Cd^(2+) (aq) hArr Fe^(2+)(aq) + Cd(s) [ Given, E_(Cd^(2+) //Cd)^(@) = - 0.40V , E_(Fe^(2+)//Fe)^(@) = - 0.44 V ]

Calculate the half cell potential at 25^@C for the cell reaction Cu^(2+)(aq)+2erarrCu , When [Cu^(2+)]=4M and E^@(Cu^(2+)//Cu)=0.34V .

The reaction, Cu^(2+)(aq) +2CI^- (aq) rarr Cu(s) +CI_2(g) has E_(cell)^@=1.03V .This reaction :