Given that the standard electrode potentials of metals are:
`K^+|K=-2.93V, Ag^+|Ag=0.80V, Cu^(2+)|Cu=0.34V, Mg^(2+)|Mg= -2.37V , Cr^(3+)/Cr=-0.74V` `Fe^(2+)|Fe=-0.44V`.
Arrange the metals in the increasing order of their reducing power.

Give the standard electrode potentials: Mg^2+ / Mg = -2.37 V, Cr^3+/Cr = - 0.74V . Arrange these metals in their increasing order of reducing power.

Arrange the metals Mg, Na, Ag, Cu, Fe, Zn in the increasing order of reactivity.

Given the standard electrode potentials: K^+/K=-2.93V . Ag^+/Ag=0.80V',Arrange these metals in their increasing order of reducing power.

1 M solution each of Cu(NO_3)_2 , AgNO_3 , Hg(NO_3)_2 and Mg(NO_3)_2 is electrolysed using Pt electrons. The values of standard reduction electrode potentials in volts are: Ag^+|Ag=+0.80V, Cu^(2+)|Cu=+0.34V Hg^(2+)|Hg=+0.79V, Mg^(2+)|Mg=-2.37V The sequence of deposition of metals on the cathode will be

Calculate the standard electrode potential of Ni2+/Ni electrode if emf of the cell Ni |Ni2+(0.01 M)||Cu2+(0.1 M)| Cu(s) is 0.59 V at 25°C [Given: Ecu2+Icu = +0.34 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 :

Calculate the e.m.f of the following cell at 298K 2Cr(s)+3Fe^(2+)(0.01M)rarr2Cr^(3+)(0.1M)+3Fe(s) Given: E^@(Cr^(3+)|Cr)=-0.75V , E^@(Fe^(2+)|Fe)=-0.45V .

Write the Nernst equation for the above cell, if E^@(Zn^(2+)|Zn)=-0.76V, E^@(Cu^(@+)|Cu)=+0.34V