Question

What mass of platinum could be plated on a electrode from the electrolysis of Pt(NO3)2 solution with a current of o.500 A for 55.0 s

Answer 1

The mass of platinum that could be plated from a Pt(NO3)2 solution using a current of 0.500 A for 55.0 s is 0.00139 g.

Step-by-step explanation:

To calculate the mass of platinum that could be plated on an electrode from the electrolysis of Pt(NO3)2 solution with a current of 0.500 A for 55.0 s, we first need to determine the number of moles of electrons that passed through the cell using the equation:

I = q/t

where I is the current in amperes, q is the charge in coulombs, and t is the time in seconds.

The total charge, q, is:

q = I × t
0.500 A × 55.0 s = 27.5 C

Then, we convert the charge to moles of electrons:

27.5 C × (1 mole e− / 96500 C) = 2.85 x 10−5 moles e−

Knowing the moles of electrons and the fact that platinum's charge during electrolysis is +4, we can find the moles of platinum plated:

2.85 x 10−5 moles e− / 4 e− per Pt = 7.13 x 10−6 moles Pt

Finally, we find the mass of platinum plated by multiplying the moles of platinum by its molar mass (195.08 g/mol):
7.13 x 10−6 moles Pt × 195.08 g/mol = 0.00139 g Pt

Therefore, the mass of platinum that could be plated is 0.00139 g.

Answer 2

The mass of platinum that could be plated on the electrode is 0.0279 g.

Step-by-step explanation:

To determine the mass of platinum that could be plated on an electrode from the electrolysis of Pt(NO3)2 solution, we need to use Faraday's law of electrolysis. Faraday's law states that the amount of substance produced at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the cell. It can be expressed as:

Amount of Substance (in moles) = (Current (in Amperes) × Time (in seconds)) / (Number of moles of electrons per mole of substance)

In this case, since platinum has a charge of +2 in the Pt(NO3)2 ion, the number of moles of electrons per mole of platinum is 2.

Using the given current of 0.500 A and time of 55.0 s, we can calculate the amount of platinum that could be plated:

Amount of Substance (in moles) = (0.500 A × 55.0 s) / 2 = 13.75 C

Since 1 mole of electrons carries a charge of 1 Faraday (F = 96500 C/mole), we can calculate the moles of platinum using the equation:

Amount of Substance (in moles) = 13.75 C / 96500 C/mole = 0.0001427 moles

The molar mass of platinum is 195.08 g/mol. Therefore, the mass of platinum that could be plated is:

Mass of Platinum = 0.0001427 moles × 195.08 g/mol = 0.0279 g