Question

During electrolysis, a metal of relative atomic mass 24.02 is deposited on the cathode, when a current of 0.152A flow for a period of 3.52 hours. Calculate the charge on the ions of the metals

Answer 1

[AI-generated answer — Bot GPT 3.5]

To find the charge on the ions of the metal being deposited during electrolysis, we first need to calculate the total charge that passed through the circuit.

Current (I) = 0.152 A
Time (t) = 3.52 hours = 3.52 hours x 3600 s/hour = 12672 s

Total charge = Current x Time
Total charge = 0.152 A x 12672 s
Total charge = 1926.144 C

Next, we need to determine the number of moles of the metal deposited on the cathode using the Faraday's law of electrolysis formula:

Q = nF

Where:
Q = Total charge passed through the circuit (in C)
n = number of moles of the metal
F = Faraday's constant = 96500 C/mol

Rearranging the formula to solve for n:

n = Q/F
n = 1926.144 C / 96500 C/mol
n = 0.01999 moles

Since the relative atomic mass of the metal is 24.02, the mass of the metal deposited on the cathode can be calculated as follows:

Mass = number of moles x Relative atomic mass
Mass = 0.01999 moles x 24.02 g/mol
Mass = 0.480 g

Finally, we can determine the charge on the ions of the metal by considering that one ion of the metal has deposited on the cathode for every electron passed through the circuit. So, the charge on the ions of the metal is equal to the total charge passed through the circuit:

Charge on ions of the metal = Total charge passed through the circuit
Charge on ions of the metal = 1926.144 C

Therefore, the charge on the ions of the metal is 1926.144 C.