Electrochemistry - Class 12 MCQ

When electricity is passed through a solution of AICI₃, 13.5 g of AI is discharged. The amount of charge passed is:    

The specific conductance of a 0.01 M solution of KCI is 0.0014 ohm-1 at 25⁰C. Its equivalent conductance is:    

The equivalent conductivity of 0.1 N CH₃COOH at 25⁰C is 80 and at infinite dilution 400 ohm^-1. The degree of dissociation of CH₃COOH is:    

One faraday of charge was passed through the electrolytic cells placed in series containing solution of Ag⁺, Ni²⁺ and Cr³⁺ respectively. The amount of Ag (At. mass 108), Ni (At. mass 59) and Cr (At mass 52) deposited will be:      

At 25⁰C, the , molar conductance at infinite dilution for the strong electrolytes NaOH, NaCI and BaCI₂ are 248 x 10^-4, 126 x 10^-4 and 280 x 10^-4 S m² mol^-1 respectively.    

The electrochemical cell stops working after some time because :    

If a spoon of copper metal is placed in a solution of ferrous sulphate :    

Which of the following represent the potential of silver wire dipped into 0.1 M AgNO₃ solution at 25⁰C ?

If the solution of the CuSO₄ in which copper rod is immersed is diluted to 10 times, the electrode potential :    

From the electrochemical series, it can be conculded that:    

Which is not true for a standard hydrogen electrode?    

Given, standard electrode potential;The standard electrode potential 

The standard electrode potential 

The potential of a hydrogen electrode at pH = 10 is:    

The standard emf for the cell reaction,

is 1.10 volt at 250C. The emf for the cell reaction when solution are used at 250C

Kohlrausch’s law states that at:    

Statements:    
(i) Unit of specific conductivity is ohm^-1 cm^-1    
(ii) Specific conductivity of strong electrolytes decreases on dilution.    
(iii) The amount of an ion discharged during electrolysis does not depend upon resistance.    
(iv) The unit of electrochemical equivalence is g/coulomb.    

The emf of the cell in which the following reaction,   occurs, is formed to 0.5105 V at 298 K. The standard emf of the cell is:

In the electrochemical reaction.   increasing the concentration of Fe²⁺:    

When 9.65 coulomb of electricity is passed through a solution of silver nitrate (Atomic mass of Ag=108 g mol^-1), the amount of silver deposited is:    

A current is passed through two voltameters connected in series. The first voltameter contains XSO₄(aq.) while the second voltameter conatins Y₂SO₄(aq.). The relative atomic masses of X and Y are in the ratio 2:1. The ratio of the mass of X liberated to the mass of Y liberated is:    

In which of the following cells will the emf be independent of the acitvity of the chloride ions?

The emf of the cell, at 298 K is 0.2905 V then the value of equilibrium constant for the cell reaction is:

The standard electrode potential of Ag⁺/ Ag is + 0.80 V and of Cu²⁺ / Cu is + 0.34 V. These electrodes are connected through a salt bridge and if:

The reduction potential of hydrogen half-cell will be negative if:

Given    The potential for the cell,  :

The emf of a cell containing sodium/ copper electrodes is 3.05 V, if the electrode potential copper electrode is +0.34 V, the electrode potential of sodium is:    

Given  

Among the following, the strongest reducing agent is: