An aqueous solution containing `Na^(+),Sn^(2+),Cl^(-) " & " SO_(4)^(2-)` ions, all at unit concentration, is electrolysed between a silver anode and a platinum cathode. What changes occur at the electrodes when current is passed through the cell ? Given : `E_(Ag^(+)|Ag)^(0)=0.799 V`
`E_(Sn^(2+)|Sn)^(@)=-0.14V, E_(Cl_(2)|Cl^(-))^(@)=1.36 V, E_(S_(2)O_(8)^(2-)|SO_(4)^(2-))^(@)=2V, E_(Sn^(4+)|Sn^(2+))^(@)=0.13V`

An aqueous solution containing Na^(+),Sn^(2+),Cl^(-) & SO_(4)^(2-) ions, all at unit concentration is electrolysed between a silver anode and a platium cathode. What changes occur at the electrodes when curret is passed through the cell? Given E_(Ag^(+)|Ag)^(0)=0.799V , E_(Sn^(2+)|Cn)^(0)=-0.14V,E_(Cl_(2)|Cr^(-))^(0)=1.36V,E_(S_(2)O_(8)^(2-)|SO_(4)^(2-))=2V,E_(Sn^(4+)|Sn^(2+))^(0)=0.13V (A). Sn^(2+) is reduced and Cl^(-) is oxidized (B). Ag is oxidized and Sn^(2+) is reduced (C). Sn^(2+) is reduced and Sn^(2+) is oxidized (D). H^(+) is reduced and Sn^(2+) is oxidised

An aqueous solution containing Na^(+),Sn^(2+),Cl^(-) & SO_(4)^(2-) ions, all at unit concentration is electrolysed between a silver anode and a platium cathode. What changes occur at the electrodes when curret is passed through the cell? Given E_(Ag^(+)|Ag)^(0)=0.799V , E_(Sn^(2+)|Cn)^(0)=-0.14V,E_(Cl_(2)|Cr^(-))^(0)=1.36V,E_(S_(2)O_(8)^(2-)|SO_(4)^(2-))=2V,E_(Sn^(4+)|Sn^(2+))^(0)=0.13V (A). Sn^(2+) is reduced and Cl^(-) is oxidized (B). Ag is oxidized and Sn^(2+) is reduced (C). Sn^(2+) is reduced and Sn^(2+) is oxidized (D). H^(+) is reduced and Sn^(2+) is oxidised

Will Sn reduce Sn^(4)+ to Sn^(2+) ? [ Given E_(Sn^(2+)|Sn)^(@)=0.14V,E_(Sn^(4+)|Sn^(2+))^(@)= 0.15 V ]

Select the correct statement if- E_(Mg^(2+)//Mg)^(@)=-2.4V, E_(Sn^(4+)//Sn^(2+))^(@)=0.1V, E_(MnO_(4)^(-),H^+//Mn^(2+))^(@)=1.5V, E_(I_(2)//I^(-))^(@)=0.5V

Select the correct statement if- E_(Mg^(2+)//Mg)^(@)=-2.4V, E_(Sn^(4+)//Sn^(2+))^(@)=0.1V, E_(MnO_(4)^(-),H^+//Mn^(2+))^(@)=1.5V, E_(I_(2)//I^(-))^(@)=0.5V

Which of the following statements is correct ? If E_(Cu^(2+)|Cu)^(@) = 0.34 V and E_(Sn^(2+)|Sn)^(@) = -0.136 V , E_(H^(+)|H_2)^(@) = -0.0V

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 .

Which of the following statements is correct? If E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Sn^(2+)|Sn)^(@)=-0.136V,E_(H^+|H_2)^(@)=-0.0V

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 .

Which of the following statements is correct? If E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Sn^(2+)|Sn)^(@)=-0.136V "and"E_(H^+|H_2)^(@)=-0.0V