Home
Class 12
CHEMISTRY
Consider the following electrolytic cell...

Consider the following electrolytic cells
(i) `M (s) | M ^(2+) (aq), 0.1 M || X ^(2+) (aq), 0.01 M |X (s)`
(ii) `M (s) | M ^(2+) (aq), 0.1 M || X ^(2) (aq), 0.01 M | X (s)`
(iii) `M (s) | M ^(2+) (aq), 0.1 M || X ^(2) (aq), 0.01 M | X (s)`
The cell EMF of the above cells are `E_(1), E _(2)` and `E_(3)` respectively. Which one of the following is true?

A

a) `E _(1) gt E _(2) gt E _(3)`

B

b) `E _(2) gt E _(3) gt E _(1)`

C

c) `E _(3) gt E _(2) gt E _(1)`

D

d) `E _(1) gt E _(3) gt E _(2)`

Text Solution

Verified by Experts

The correct Answer is:
D

For te given cell, cell reaction is
`M + X ^(2+) to M ^(2+) + X`
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the e.m.f of the following concentration cell at 298K, Zn(s)| Zn^(2+)(0.1) || Zn^(2+) (1.0)|Zn(s)

For the cell Zn|Zn^(2+)(0.01M)||M_((0.001M))^(2+)|M,E_("cell")=0.29V . When Q=K_(eq) , which of the following is true?

For the following electrochemical cell at 298 K Pt (s)|H_2(g) (1 ba r) |H^+ (aq) 1M||M^(4+) (aq) , M^(2+) (aq)|Pt(s) E_(cell)=0.092 V when ([M^(2+)])/([M^(4+)])=10^x Given: E_(M^(4+),M^(2+))^@=0.151V, 2.303 (RT)/F=0.059 The value of x is

E_("cell") of the following is Pt(s)|H_(2)(g), 1 "bar" |H^(+)(1M)||H^(+) (0.1 M)| H_(2)(g), I " bar" |Pt(s)

If the solubility of AgCl in H_(2)O, 0.1M CaCl_(2), 0.01M KCl and 0.02M AgNO_(3) " are " S_(1), S_(2), S_(3) and S_(4) respectively, the correct order of solubility are

E_(cell)^@ for Zn(s)+Pb^(2+) (1M ) to Zn^(2+) (1M) +Pb(s) is 0.66 volt. E_(cell) for the reaction Zn(s)+Pb^(2+) (0.1M) to Zn^(2+) (0.1M) +Pb(s) is

Suppose the solubilities of AgCl in water, in 0.01 M CaCl_(2) solution, in 0.01 M NaCl solution and in 0.05 M AgNO_(3) solution are S_(1), S_(2), S_(3) and S_(4) respectively. The correct order of these solubilities is

Write the Nernst equation and emf of the following cells at 298 K. Mg_(s)// Mg^(2+) (0.001M) II Cu(2+)(0.001M)// Cu_(s), E^0cell = 2.71 V .