Home
Class 12
CHEMISTRY
An aqueous solution containing 1 M each ...

An aqueous solution containing 1 M each of `Au^(3+),Cu^(2+),Ag^+,Li^+` is being electrolysed by using inert electrodes. The value of standard reduction potentials are:
`E_(Ag+//Ag)^(@)=0.8V,E_(Cu2+//Cu)^(@)=0.34V"and" E_(Au3+//Au)^(@)=1.50V,E_(Li+//Li)^(@)=-3.03V`
with increase voltage , the squence of deposition of metals on the cathode will be:

Text Solution

Verified by Experts

Let us see if copper reacts with silver nitrate or not. If it reacts, the coppers spoon cannot be used to stir a solution of silver nitrate.
Copper will react (if possible) with silver nitrate solution as follows:
`Cu(s)+2AgnO_(3)(aq) to Cu(NO_(3))_(2)(aq)+2Ag(s)`
Or `Cu(s)+2Ag^(+)(aq)toCu^(2+)[ag+2Ag(s)](aq)`
The two half cell reactions are as follows:
`Cu(s)toCu^(2+)(aq)+Ze^(-)`
`2Ag^(+)(aq)+2e^(-) to 2Ag(s)`
The cell representing this redox reaction is:
`Cu|Cu^(2+)(aq)||Ag^(+)|Ag`
`EMF^(@)=E^(@)(Ag^(+)//Ag)-E^(@)(Cu^(2+)//Cu)`
`=+0.80V-(0.34V)=0.46V`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    BETTER CHOICE PUBLICATION|Exercise NERNST EQUATION|4 Videos

  • ELECTROCHEMISTRY

    BETTER CHOICE PUBLICATION|Exercise CONDUCTANCE OF ELECTROLYTIC SOLUTIONS|21 Videos

  • ELECTROCHEMISTRY

    BETTER CHOICE PUBLICATION|Exercise Numerical Problems|69 Videos

  • CO-ORDINATION COMPOUNDS

    BETTER CHOICE PUBLICATION|Exercise QUESTION FROM PREVIOUS BOARD EXAMINATION|59 Videos

  • GENERAL PRINCIPLES AND PROCESS OF ISOLATION OF ELEMENTS

    BETTER CHOICE PUBLICATION|Exercise Question Bank (6.6 OXIDATION-REDUCTION)|15 Videos

Similar Questions

Explore conceptually related problems

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 :

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

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

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

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

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.