Every question from past board papers on Electrolytic and galvanic cells, electrode potentials, newest paper first. Open any question for its full worked answer.
Match List I with List II.
List I (Conversion): A. 1 mol of \(H_2O\) to \(O_2\) B. 1 mol of \(MnO_4^-\) to \(Mn^{2+}\) C. 1.5 mol of Ca from molten \(CaCl_2\) D. 1 mol of FeO to \(Fe_2O_3\)
List II (Number of Faraday required): I. 3F II. 2F III. 1F IV. 5F
Choose the correct answer from the options given below:
Mass in grams of copper deposited by passing 9.6487 A current through a voltmeter containing copper sulphate solution for 100 seconds is:
(Given : Molar mass of Cu : 63 g \(mol^{-1}\), 1F = 96487 C)
At 298 K, the standard electrode potentials of \(Cu^{2+}/Cu\), \(Zn^{2+}/Zn\), \(Fe^{2+}/Fe\) 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 can not occur ?
On electrolysis of dil.sulphuric acid using Platinum (Pt) electrode, the product obtained at anode will be :
The number of Faradays(F) required to produce 20 g of calcium from molten CaCl\(_2\) (Atomic mass of Ca = 40 g mol\(^{-1}\)) is :
The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is (charge on electron = \(1.60\times10^{-19}\) C)
Zinc can be coated on iron to produce galvanized iron but the reverse is not possible. It is because
During the electrolysis of molten sodium chloride, the time required to produce \(0.10\) mol of chlorine gas using a current of 3 amperes is
