The following chemical reaction is occuring in an electro-chemical cellMg(s) + 2Ag+(0.001 M) → Mg2+(0.10 M) + Ag(s)The E° electrode values areMg2/Mg = – 2.36 VAg+/Ag = 0.81V For the cell calculate/write:(a) (i) E° value for the electrode 2Ag+/2Ag(ii) Standard cell potential E°Cell(b) Cell potential (E)cell(c) (i) Symbolic representation of the above cell     (ii) Will the above cell reaction be spontaneous?   from Chemistry Electrochemistry Class 12 Nagaland Board
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Class 10 Class 12
The following chemical reaction is occuring in an electro-chemical cell
Mg(s) + 2Ag+(0.001 M) → Mg2+(0.10 M) + Ag(s)
The E° electrode values are
Mg2/Mg = – 2.36 V
Ag+/Ag = 0.81
V For the cell calculate/write:
(a) (i) E° value for the electrode 2Ag+/2Ag
(ii) Standard cell potential E°Cell
(b) Cell potential (E)cell
(c) (i) Symbolic representation of the above cell
     (ii) Will the above cell reaction be spontaneous?
 

Mg(s) → Mg2+(aq) + 2e
2Ag+(aq) + 2e → 2Ag(s)

Mg(s) +2Ag+(aq)  Mg2+(aq) +2Ag(s)The cell may be represented as Mg I Mg2+(0.10M)Ag+(0.001)M I Aga) Ecell0 = EAg+Ag0 - EMg2+Mg0   =+0.81V -(-2.36V)   = +0.18V +2.36   =3.17Vb) Ecell = Ecell0 - 0.05912log [Mg2+][Ag+]2Ecell =+3.17V-0.05912log0.10(0.001)2   =3.17V -0.05912log 0.10×108   = 3.17-0.02955×(8-1)V   = 3.17-0.02955×7V   = 3.17-0.21V =2.96C) Mg I Mg2+(0.10M)Ag+(0.001)M I Agsince the  Standard cell potential Ecell0 is positive   Ecell0 = EAg+Ag0 - EMg2+Mg0   =+0.81V -(-2.36V)   = +0.18V +2.36   =3.17Vthus reaction is spontaneous
190 Views

How would you determine the standard electrode potential of the system Mg2+/Mg?

Answer:

Use standard hydrogen electrode as anode and Mg2+ | Mg as a cathode we can measure the standard electrodepotential of systemMg2+ | Mg. Standard hydrogen electrode, represented by Pt(s), H2(g) (1 atm) | H+ (aq) and dip the electrode of Magnesium wire in a 1M MgSO4 solution .The standard hydrogen electrode is always zero.
Use formula
Eocell = Eo right  – Eoleft
The standard hydrogen electrode is always zero.
So that the value of
Eoleft =0
Hence
Eocell = Eo Mg|Mg2+
Or
Eo Mg|Mg2+= Eocell
2203 Views

Consult the table of standard electrode potentials and suggest three substance that can oxidize ferrous ions under suitable conditions.

Answer:


oxidation of ferrous ion means :

Fe2+--> Fe3+ +e-EFe3+Fe2+0 = 0.77V
Any substance which standard electrode potential is more than that of Fe+3 /F+2 can oxidise ferrous ions. 
(refer to the table given in book)

The EMF of the substance whose reduction potentials greater than 0.77V will oxidised ferrous ion.
for example Br2, Cl2,and F2 .

879 Views

Calculate the emf of the cell in which the following reaction takes place:
Ni(s) + 2Ag+ (0.002 M)  Ni2+ (0.160 M) + 2Ag(s)
Given that EoCell = 1.05 V

Answer:

Ni(s)+2Ag+(aq)Ni2+(aq)+2As(s)
Ecell = Eocell + RT2FlnAg+(aq)2Ni2+ (aq)
or      Ecell = Eocell+0.0592 logAg+(aq)2Ni2+ (aq)
 
The equation is also written as

or    Ecell = Eocell-0.0592logNi2+(aq)Ag+ (aq)2         = 1.05 V - 0.0295 log 0.1600.002  

= 1.05 V – 0.0295 x log 80

= 1.05 V – 0.0295 x 1.9031

= 1.05 V – 0.056 = 0.99 V.

1585 Views

Calculate the potential of hydrogen electrode in contact with a solution whose pH is 10.

Answer:

For hydrogen electrode, ,
given that      pH = 10
use formula [H+] = 10–pH
so that  [H+] = 10−10 M
Electrode reaction will
H+  + e –  →1/2 H2
Use the formula


EH+/H2  = EoH+/H2 - RTnFlnH2[H+]2              = 0-8.314×2982×96500ln IH+2              = 0.05915 log [H+]              =-0.05915 pH             =-0.05915 × 10 =- 0.59 V
1279 Views

Can you store copper sulphate solutions in a Zinc pot?

Answer:

No. Because zinc is more reactive than copper and thus holes will be developed in zinc pot.

Cu2+(aq) + Zn(s) → Zn2+ (aq) + Cu(s)
1384 Views