Using the given data ,find the strongest reducing agent
`E^@Cr^(6+)//Cr^(3+)=1.33V,E^@Cl_2//Cl^(-)=1.36V`
`E^@ Mn^(7+)//Mn^(2+)=1.51 V, E^(@) Cr^(3+)//Cr =-0.74 V. `

Can Chlorine gas be stored in Copper Cylinder ? Given E_(Cu^(+)//Cu)^(@)= 0.34V and E_(Cl_(2)//Cl)^(@)= 1.36V

Based on the data, arrange Fe^(2+), Mn^(2+) and Cr^(2+) in the increasing order of stability of +2 oxidation state: E_(Cr^(3+)//Cr^(2+))^0= -0.4V, E_(Mn^(3+)//Mn^(2+))^0= 1.5V, E_(Fe^(3+)//Fe^(2+))^0= 0.8V

Write NERNST equation also Calculate the cell e.m.f. and DeltaG for the cell reaction at 25^(@)C Cr(s)//Cr^(3+)(0.1M)"//"Fe^(2+)(0.01M)//Fe(s) Given E_(Cr^(3+)//Cr)^(0)=-0.75V, E_(Fe^(2+)//Fe)^(0)=-0.45V

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 reduction potential of the following electrode at 298K Pt,Cl_2(2.5atm)|HCl(0.01M), E^@ Cl_2|2Cl^-=1.36V .

Find the oxidation number of central atom : [Cr(NH_3)_4Cl_2]^(+)

When a solution of AgNO_3 (1 M) is electrolysed using platinum anode and copper cathode, what are the products obtained at two electrodes? Given : E_(cu^(2+)|cu)^(@)=+0.34 V , E_(H_2O|O_2,H^+)^(@)=-1.23 V E_(H^+|H_2)^(@)=+0.0V , E_(ag^+|Ag)^(@)=+0.8 V

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

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.