List of top Chemistry Questions on Electrolytic Cells and Electrolysis

A solution of copper sulphate is electrolysed for \(10\) minutes with a current of \(1.5\) ampere. The mass of copper deposited at the cathode is: \[ \text{Given: Molar mass of Cu}=63.5\text{ g mol}^{-1} \] \[ F=96487\text{ C mol}^{-1} \]

Conductivity of CH\(_3\)COOH decreases on dilution. 

On the basis of \( E^\circ \) values, O\(_2\) gas should be liberated at the anode, but it is Cl\(_2\) gas that is liberated in the electrolysis of aqueous NaCl.
Explain Faraday’s First Law of Electrolysis

State the following:
Kohlrausch law of independent migration of ions 

The reactions taking place during electrolysis of aqueous solution of CuCl2 with platinum electrodes are :
A. Cu2+(aq) + 2e- → Cu(s)
B. H+(aq) + e- → \(\frac{1}{2}H_2(g)\)
C. H2O(l) + e- → \(\frac{1}{2}H_2(g)+^-OH(aq)\)
D. Cl-(aq) → \(\frac{1}{2}Cl_2(g)+e^-\)
E. 2-OH(aq) → H2O(l) + \(\frac{1}{2}O_2(g)+2e^-\)
Choose the correct answer from the options given below :
If we use molten NaCl, the products of electrolysis are ____.