If `E_(Au^(+)//Au)^(@)` is 1.69 V and `E_(Au^(3+)//Au)^(@)` is 1.40 V, then `E_(Au^(+)//Au^(3+))^(@)` will be :

An aqueous solution containing 1M each of Au^(3+), Cu^(2+), Ag^(+), Li^(+) is being electrolysed by using inert electrodes. The value of standard potentials are E_(Ag^(+)//Ag)^(@)= 0.80V, E_(Cu^(2+)//Cu)^(@) = 0.34V, and E_(Au^(3+)//Au)^(@) = 1.50 V , E_(Li^(+)//Li)^(@)= -3.03V , With increasing voltage, the sequence of deposition of metals on the cathode will be

Arrange the following metals in increasing order of their reducing power. [ Given : E_(K^(+)//K)^(@)=-2.93V, E_(Ag^(+)//Ag)^(@)=+0.80V, E_(Al^(3)//Al)^(@)=-1.66V, E_(Au^(3+)//Au)^(@)=+1.40 V, E_(Li^(+)//Li)^(@)=-3.05 V ]

Four different solution containing 1M each of Au^(+3), Cu^(+2), Ag^(+), Li^(+) are being electrolysed by using inert electrodes. In how many samples, metal ions would be deposited at cathode? ["Given :" E_(Ag^+//Ag)^(0) = 0.8, E_(Au^(+3)//Au)^(0) = 1.00 V E_(Cu^(+2)//Cu)^(0) = 0.34 V, E_(Li^(+)//Li)^(0)= -3.03 V ]

Four different solution containing 1M each of Au^(+3), Cu^(+2), Ag^(+), Li^(+) are being electrolysed by using inert electrodes. In how many samples, metal ions would be deposited at cathode? ["Given :" E_(Ag^+//Ag)^(0) = 0.8, E_(Au^(+3)//Au)^(0) = 1.00 V E_(Cu^(+2)//Cu)^(0) = 0.34 V, E_(Li^(+)//Li)^(0)= -3.03 V ]

An aqueous solution containing 1M each of Au^(3+),Cu^(2+),Ag^(+),Li^(+) is being electrolysed by using inert electrodes. The value of standard potentials are : E_(Ag^(+)//Ag)^(@)=0.80 V,E_(Cu^(+)//Cu)^(@)=0.34V and E_(Au^(+3)//Au)^(@)=1.50,E_(Li^(+)//Li)^(@)=-3.03V will increasing voltage, the sequence of deposition of metals on the cathode will be :

An aqueous solution containing 1M each of Au^(3+),Cu^(2+),Ag^(+),Li^(+) is being electrolysed by using inert electrodes. The value of standard potentials are : E_(Ag^(+)//Ag)^(@)=0.80 V,E_(Cu^(+)//Cu)^(@)=0.34V and E_(Au^(+3)//Au)^(@)=1.50,E_(Li^(+)//Li)^(@)=-3.03V will increasing voltage, the sequence of deposition of metals on the cathode will be :