Electrochemistry- Test 01

for the cell reaction
$$Cu^{2+}(C_1aq)+Zn(s)=Zn^{2+}(C_2aq)+Cu(s)$$
of an electrochemical cell, the change in free energy at a given temperature is a function of 

The main reason for not using a mercury electrolytic cell in NaOH manufacture is that 

In which cell the free energy of a chemical reaction is directly converted into electricity 

$$E^o_{Cell}$$ for some half-cell reactions are given below. On the basis of these mark the correct answers.

$$E_n = -\dfrac{313.6}{n^2}$$, if the value of $$E_i = -38.84$$ to which value 'n' corresponds?

Two electrolytic cells containing $$CuSO_{4}$$ and $$AgNO_{4}$$ respectively are connected in series and a current is passed through them unit 1 mg of copper is deposited in the first cell. The amount of silver deposited in the second cell during this time is approximately 
[ Atomic weight of copper and silver are respectively 63.57 and 107.88] 

Resistance of a voltameter is 2$$\Omega $$, it is connected in series to a battery of 10 V through a resistance of 3$$\Omega $$ . In a certain time mass deposited on cathode is 1 gm. Now the voltameter and the 3$$\Omega $$resistance are connected in parallel with the battery. Increase in the deposited mass on cathode in the same time will be

If redox reaction takes place in cell then electromotive force (e.m.f) of cell will be:

Which of the following mixtures represents rusting of iron?

The amount of charge required to liberate 9 gm of aluminium ( atomic weight = 27 and valency = 3 ) in the process of electrolysis is ( Faraday's number = 96500 coulombs/gm equivalent)