E.M.F of the cell reaction , 2Ag^(+) + Cu to 2Ag + Cu^(2+) is 0.46 V . If E_(Cu^(2+) // Cu)^(0) is | 0.34 V , E_(Ag^(+)//Ag)^(0) is
E_("red")^(0) (Standard reduction potential ) of different half-cells are given E_(Cu^(+2)//Cu)^(0) = 0.34 V E_(Zn^(+2)//Zn)^(0) = -0.76 V , E_(Ag^(+) // Ag)^(0) = 0.80 V , E_(Mg^(2+) // Mg)^(0) = -2.37 V . In which cell DeltaG^(@) is most negative ?
E_(Al^(3+)//Al)^0 =- 1.66 V and E_(Tl^(3+)//Tl)^0 = 1.26 V. Then which of the following statements is correct ?
Given E_(Ag^(+) // Ag)^(0) = 0.80 V , E_(Mg^(2+) // Mg)^(0) =-2.37 V , E_(Cu^(2+) // Cu)^(0) = 0.34 E_(Hg^(2+) // Hg)^(0) = 0.79 V Which of the following statement is / are correct ?
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
E_(cell)^(@) is 1.89V for the reaction 2Ce^(4+) +Co rarr 2Ce^(3+)+Co^(2+) . If E_(Co^(2+)//Co) is -0.28V . What is the value of E_(Ce^(4+)//Ce^(3+))^(@) ?
Cu^+ ion is not stable in aqueous solution because of diproportionation reaction . E^(@) value for the disproportionation of Cu^(+) is : (E_(cu^(2+)// cu^+)^(@) = + 0.15 V , E_(cu^(+) // cu)^(@)= + 0.34 V )
Copper reduces NO_3^(-) into NO and NO_2 depending upon concentration of HNO_3 in solution . Assuming [Cu^(2+)] = 0.1 M , and P_(NO) = P_(NO_2) = 10^(-3) bar . At which concentration of HNO_3 . Thermodynamic tendency for reduction of NO_3^(-) into NO and NO_2 by copper is same ? Given : E_(Cu^(2+)|Cu)^(@) = + 0.34 V , E_(NO_3^(-)|NO)^(@) = + 0.96 V , E_(NO_3^(-)|NO_2)^(@) = + 0.79 V
