Question

29.1 What volume (cm) and weight (g) of zinc will be deposited onto a cathodic workpart if 10 amps of current are applied for one hour?

Answer 1

The process which is basically used in this problem is called Electroplating technique,

As per this process,the workpart which is to be coated with zinc is called cathode and anode is the metal part (zinc) here. These both parts are immersed in Electrolytic solution which allows flow of Electricity.The Direct power supply is given to anode which will oxidise metal atoms and will dissolve in the Electrolyte solution. The dissolved metal ions will deposit on cathode.

The Formula for solving the problem is given below.

Volume (cm3) of zinc will be deposited if 10amp current applied for 1hr:

V= E*C*I*t

E = Cathode Efficency (%) for Zinc 95% (Standard Value for Zinc deposition in Chloride Electrolyte)

C Plate Constant = 4.75X10^-2 mm3/sec

I Current =10 Amp

t = 1hr =>1*60*60=>3600Sec

V= .95X4.75X10^-2*10*3600

= 1624.5mm3

In order to calculate Volume of zinc will be deposited in cm3 we need to multiply by 0.001(1mm=0.1cm)

V = 1624.5x .001 =>1.6245cm3

Density of Zinc = 7.15gm/cm3(Standard Value)

We Know Density = Weight/Volume

Weight = Density X Volume

= 7.15 X 1.6245

= 11.6152 grams

Weight of zinc will be deposited in 1 hr by passing 10Amp Current = 11.6152 Grams