List of top Chemistry Questions on Electrochemistry asked in BITSAT

The standard electrode potential for $\text{Zn}^{2+}/\text{Zn}$ is $-0.76$ V and for $\text{Cu}^{2+}/\text{Cu}$ is $+0.34$ V. The EMF of the cell
$$ \text{Zn}|\text{Zn}^{2+}||\text{Cu}^{2+}|\text{Cu} $$ is:
The standard reduction potentials are: \[ \mathrm{Cu^{2+} + 2e^- \rightarrow Cu} \quad E^\circ = +0.34\,V \] \[ \mathrm{Zn^{2+} + 2e^- \rightarrow Zn} \quad E^\circ = -0.76\,V \] Calculate the standard cell potential for the reaction: \[ \mathrm{Zn + Cu^{2+} \rightarrow Zn^{2+} + Cu} \]
In the electrolysis of molten \( \mathrm{NaCl} \), what is produced at the cathode?
Specific conductance of 0.1M HA is 3.75 × 10⁻4Ω⁻1cm⁻1. If Lambdam^∘(HA) = 250Ω^-1cm²mol⁻1, the dissociation constant Kₐ of HA is
Stronger is oxidising agent, more is
Which of the following relation represents correct relation between standard electrode potential and equilibrium constant? I. log K = (nF E^∘)/(2.303RT) II. K = e⁽ⁿF E^∘⁾/⁽RT⁾ III. log K = (-nF E^∘)/(2.303RT) IV. log K = (0.4342 nF E^∘)/(RT) Choose the correct statement(s).
Electrolysis is carried out in three cells:
The mass of the substance deposited when one Faraday of charge is passed through its solution is equal to
On passing a current of 1.0A for 16 min and 5 s through one litre of CuCl₂ solution, all copper of the solution was deposited at cathode. The strength of the CuCl₂ solution was (Molar mass of Cu = 63.5; Faraday constant = 96,500C mol⁻1):
A 100.0mL dilute solution of Ag⁺ is electrolysed for 15.0 minutes with a current of 1.25mA and the silver is removed completely. What was the initial [Ag⁺]?

Which of the following relations represents the correct relation between standard electrode potential and equilibrium constant?

I. \(\log K = \frac{n F E^\circ}{2.303 R T}\)

II. \(K = e^{\frac{n F E^\circ}{R T}}\)

III. \(\log K = -\frac{n F E^\circ}{2.303 R T}\)

IV. \(\log K = 0.4342 \frac{n F E^\circ}{R T}\)

Choose the correct statements.

Specific conductance of 0.1 M \(HA\) is \(3.75 \times 10^{-4} \, \Omega^{-1} \text{cm}^{-1}\). If \(\Lambda_m^\infty (HA) = 250 \, \Omega^{-1} \text{cm}^2 \text{mol}^{-1}\), the dissociation constant \(K_a\) of \(HA\) is
Electrolysis is carried out in three cells: (A) 1.0M CuSO₄ using Pt electrodes (B) 1.0M CuSO₄ using Cu electrodes (C) 1.0M KCl using Pt electrodes If volume of electrolyte solution is maintained constant in each cell, which is the correct set of change of pH in the (A), (B) and (C) cell respectively?
The efficiency of fuel cell is given by the expression \(\eta\) is:
The mass of the substance deposited when one Faraday of charge is passed through its solution is equal to:
The electrolytic cells, one containing acidified ferrous chloride and another acidified ferric chloride are connected in series. The ratio of iron deposited at cathodes in the two cells when electricity is passed through the cells will be:
A current of 2.0 A passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At wt. = 177). The oxidation state of the metal in the salt is
The ionic conductance of \( \text{Ba}^{2+} \) and \( \text{Cl}^- \) respectively are 127 and 76 \( \text{S} \, \text{cm}^{-1} \) at infinite dilution. The equivalent conductance of \( \text{BaCl}_2 \) at infinite dilution will be:
Which of the following cannot give iodometric titration?
The number of coulombs required for the deposition of 108 g of silver is:
A gas X at 1 atm is bubbled through a solution containing a mixture of 1 M Y^- and 1 M Z^+ at 25C. If reduction potential is Z > Y > X, then: