In an electrolysis experiment a cathode of mass 4.5g weighs 4.52g after a current of 4.5A flows for 1hrs.The electrochemical equivalent of the deposited substance is ?

To find the electrochemical equivalent of the deposited substance, we first need to calculate the amount of substance deposited on the cathode.

The change in mass of the cathode is 4.52g - 4.5g = 0.02g.

Next, we convert the change in mass to grams per second:
0.02g / (1hr x 3600s/hr) = 5.56 x 10^-6 g/s

Now, we can calculate the charge passed through the cathode using the formula Q = I x t, where Q is the charge, I is the current, and t is the time:
Q = 4.5A x 1hr x 3600s/hr = 16200 C

Since 1 Faraday (F) is equal to 96485 C, we can calculate the number of Faradays passed through the cathode:
16200 C / 96485 C/F = 0.168 F

Finally, we can calculate the electrochemical equivalent of the deposited substance using the formula:
Electrochemical equivalent = Change in mass / (Charge x Faraday)
Electrochemical equivalent = 5.56 x 10^-6 g/s / (0.168 F x 96485 C/F) = 3.6 x 10^-8 g/C

Therefore, the electrochemical equivalent of the deposited substance is 3.6 x 10^-8 g/C.