Are the following reactions spontaneous?
(b) `Cd+Cl_(2)rarr Cd^(2+)+2Cl^(-)` `"Given : "E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Mg^(2+)|Mg)^(@)=-2.37V,`
`E_(Cd^(2+)|Cd)^(@)=-0.40V, E_((1)/(2)Cl_(2)|Cl^(-))^(@)=+1.36V`

Are the following reactions spontaneous? (a) Fe+Mg^(2+)rarr Fe^(2+)+Mg "Given : "E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Mg^(2+)|Mg)^(@)=-2.37V, E_(Cd^(2+)|Cd)^(@)=-0.40V, E_((1)/(2)Cl_(2)|Cl^(-))^(@)=+1.36V

Will the following reaction be spontaneous under standard conditions? (a) Fe+Mg^(2+)rarr Fe^(2+) +Mg (b) Cd+Cl_(2)rarrCd^(2+)+2Cl^(-) ["Given : "E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Mg^(2+)|Mg)=-2.37V, E_(Cd^(2+)|Cd)^(@)=-0.40V, E_((1)/(2)Cl_(2)|Cl^(-))^(@)=+1.36V]

Represent symbolically the galvanic cells in which the following reaction occurs. Calculate the standard electromotive forces of the cells : (2) Fe+Sn^(2+)rarr Fe^(2+)+Sn Given : E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Sn^(2+)|Zn)^(@)=-0.14V , E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V , E_(H^(+)|(1)/(2)H_(2))^(@)=0.00V .

Represent symbolically the galvanic cells in which the following reaction occurs. Calculate the standard electromotive forces of the cells : (1) Fe+CuSO_(4)rarr FeSO_(4)+Cu Given : E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Sn^(2+)|Zn)^(@)=-0.14V , E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V , E_(H^(+)|(1)/(2)H_(2))^(@)=0.00V .

Represent symbolically the galvanic cells in which the following reaction occurs. Calculate the standard electromotive forces of the cells : (3) Zn+H_(2)SO_(4)rarr ZnSO_(4)+H_(2) Given : E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Sn^(2+)|Zn)^(@)=-0.14V , E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V , E_(H^(+)|(1)/(2)H_(2))^(@)=0.00V .

It the reaction, 2Ag(s)+Fe^(2+)(aq)rarr2Ag^(+)(aq)+Fe(s) possible? Given : E_(Fe^(2+)|Fe)^(@)=-0.44V and E_(Ag^(+)|Ag)^(@)=+0.80V .

State with reason whether the following reaction is spontaneous or not : Sn^(2+)+2Fe^(3+)rarr Sn^(4+)+2Fe^(2+) ["Given, "E_(Fe^(3+)|Fe^(2+))^(@)=+0.77V, E_(Sn^(4+)|Sn^(2+))^(@)=+0.15V]

Calculate cell potential of Fe|Fe^(2+)(a=0.6)||Sn^(2+)(a=0.2)|Sn Given : E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Sn^(2+)|Sn)^(@)=+0.14V

Find the stronger oxidising agent in each pair, stating reason. (a) Cl_(2), Br_(2) "Given : "E_((1)/(2)Cl_(2)|Cl^(-))^(@)=+1.36V, E_((1)/(2)Br_(2)|Br^(-))^(@)=+1.07V, E_(Cu^(2+)|Cu)^(@)=+0.34V, E_(Ag^(+)|Ag)^(@)=+0.80V, E_(Pb^(2+)|Pb)^(@)=-0.13V, E_(Fe^(2+)|Fe)^(@)=-0.44V , E_(Fe^(3+)|Fe)^(@)=-0.036V, E_(Cr^(3+)|Cr)^(@)=-0.74V

Identify X^(-) In the following spontaneous reactions Cl_(2)+2X^(-)+X_(2) , where X^(-) is a halide ion . [ Given E_((F_(2))|2F^(-))^(@)= +2.87 V , E_(Cl_(2)|2Cl^(-))^(@) = +1.36 V, E_(Br_(2)|2Br^(-))^(@)=+1.06 V and E_(I_(2)|2I^(-))^(@)=+0.54 ]