List of top Chemistry Questions on Electrochemistry asked in NEET (UG)

If the molar conductivity ($\Lambda_m$) of a 0.050 mol $L^{–1}$ solution of a monobasic weak acid is 90 S $cm^{2} mol^{–1}$, its extent (degree) of dissociation will be:
[Assume: $\Lambda^0$ = 349.6 S $cm^{2} mol^{–1}$ and $\Lambda^0_{\text{acid}}$ = 50.4 S$ cm^{2} mol^{–1}$]

The conductivity of centimolar solution of KCI at 25°C is 0.0210 ohm-1cm-1 and the resistance of the cell containing the solution at 25°C is 60 ohm. The value of the cell constant is :
Given below are two statements labeled Assertion A and the labeled as Reason R : 
Assertion A: In the equation \(\Delta_rG=-nFE_{cell}\) value of \(\Delta_rG\) depends on n. 
Reasons R: \(E_{cell}\) is an intensive property and \(\Delta_rG\) is an extensive property. 
In the light of the above statements, choose the correct answer from the options below :

Find the emf of the cell

Ni(s) + 2 Ag+ (0.001 M) → Ni2+ (0.001 M) + 2Ag(s)

(Given that E°cell = 1.05 V, \(\frac{2.303RT}{F} = 0.059\) at 298 K)

At 298 K, the standard electrode potentials of Cu2+/Cu, Zn2+/Zn, Fe2+/Fe and Ag+/Ag are 0.34 V, - 0.76 V, - 0.44 V and 0.80 V, respectively.
On the basis of standard electrode potential, predict which of the following reaction cannot occur?
Given below are half-cell reactions:
\(MnO_4^- + 8H^+ + 5e^- → Mn^{2+} + 4H_2O\),
\(E°_{(Mn^{+2}/MnO_4^-)} = –1.510 V\)
\((\frac{1}{2})O_2 + 2H^+ + 2e^- → H_2O,\)
\(E°(O_2/H_2O) = +1.223 V\)
Will the permanganate ion, \(MnO_4^-\) liberate \(O_2\) from water in the presence of an acid?
On electrolysis of dil.sulphuric acid using Platinum (Pt) electrode, the product obtained at anode will be:
In which case change in entropy is negative? (1)(2) (3 (4)
In the electrochemical cell :
\(Zn|ZnSO_4(0.01M)||CuSO_4(1.0 M)|Cu,\)
the emf of this Daniel cell is \(E_1\). When the concentration of \(ZnSO_4\) is changed to 1.0 M and that of \(CuSO_4\) changed to 0.01 M, the emf changes to \(E_2\). From the following, which one is the relationship between \(E_1\) and \(E_2\)?
(Given, \(\frac {RT}{F}= 0.059\))
Extraction of gold and silver involves leaching with CN– ion. Silver is later recovered by
The weight of silver (at wt. = 108) displaced by a quantity of electricity which displaces 5600 mL of O2 at STP will be:
When 0.1 mol MnO42– is oxidised the quantity of electricity required to completely oxidise MnO42– to MnO4– is
At 25°C molar conductance of 0.1 molar aqueous solution of ammonium hydroxide is 9.54 ohm-1 cm2 mol-1 and at infinite dilution its molar conductance is 238 ohm-1 cm2 mol-1. The degree of ionisation of ammonium hydroxide at the same concentration and temperature is
A button cell used in watches functions as following
Zn(s) + Ag2O(s) + H2O(l) ⇌ 2Ag(s) + Zn2+ (aq) + 20H- (aq)
If half cell potentials are
Zn2+(aq) + 2e- → Zn(s); E° = -0.76 V
Ag2O(s) + H2O(l) + 2e- → 2Ag(s) + 20H-(aq),
E° = 0.34 V
The cell potential will be
The standard e.m.f. of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25ºC. The equilibrium constant of the reaction would be
On the basis of the information available from the reaction: \(\frac 43 Al+O_2→\frac 23 Al_2O_2\), ∆G = -827 KJ mol-1 of O2, the minimum e.m.f. required to carry out electrolysis of Al2O3 is (F = 96500 C mol–1)
According to the Faraday Law of electrolysis, the mass deposited at electrode proportional to:
At infinite dilution equivalent conductances of \(Ba^{2+}\) & \(Cl^–\) ions are  \(127\)  & \(76\) \(ohm^{–1}cm^{–1}eq^{–1}\) respectively. Equivalent conductance of \(BaCl_2\) at infinite dilutions is:
\(\text {For\  the\  disproportionation\  of \ copper:}\) \(2Cu+→Cu^{+2}+Cu\), \(Eº\) \(\text {is:}\)
\((\text {Given \ Eº  \ for }\ Cu^{+2}/Cu \ \text {is}\  0.34\ V\ \text { and\   Eº \ for} \ Cu^{+2}/Cu^+\ \text { is}\  0.15\ V)\)
On heating one end of a piece of a metal, the other end becomes hot because of