Question

In an electrolysis bath for 24 minutes with a current of 6.5 Amps, how many grams of zinc will be plated out?

A. 6.34g of Zn
B. 3.17g of Zn
C. 12.68g of Zn
D. 1.09g Zn

Answer 1

To calculate the amount of zinc that will be plated out during electrolysis, we can use Faraday's law of electrolysis. The formula is: Mass of substance = (Current x Time x Atomic weight) / (Number of electrons x Faraday's constant). Plugging in the given values, the mass of zinc is 6.34g. Therefore, the correct answer is option A. 6.34g of Zn.

Step-by-step explanation:

To calculate the amount of zinc that will be plated out during electrolysis, we can use Faraday's law of electrolysis. The formula is:

Mass of substance = (Current x Time x Atomic weight) / (Number of electrons x Faraday's constant)

In this case, the current is 6.5 Amps and the time is 24 minutes. The atomic weight of zinc is 65.38 g/mol. The number of electrons involved in the reaction is 2 (from Zn2+ to Zn). Faraday's constant is 96,485 C/mol.

Plugging in the values:

Mass of zinc = (6.5 A x 24 min x 65.38 g/mol) / (2 x 96,485 C/mol)

Mass of zinc = 6.34 g

Therefore, the correct answer is option A. 6.34g of Zn.