Question

How many grams of silver can form by passing 19.8 A through an electrolytic cell containing silver ions for 13.2 min?

Answer 1

To determine the amount of silver formed in an electrolytic cell, you can use the equation: moles of silver = (current x time) / (Faraday's constant x charge on silver ions). After calculating the moles of silver, you can convert it to grams by multiplying it by the molar mass of silver.

Step-by-step explanation:

To determine the amount of silver formed, you can use the equation:

moles of silver = (current x time) / (Faraday's constant x charge on silver ions)

First, convert the current to coulombs by multiplying it by the time in seconds. Then, divide the coulombs by Faraday's constant (which is 96,485 C/mol of electrons) and the charge on silver ions (which is +1).

So, moles of silver = (19.8 A x 13.2 min x 60 s/min) / (96,485 C/mol x 1)

After calculating the moles of silver, you can convert it to grams by multiplying it by the molar mass of silver, which is 107.87 g/mol.

Therefore, the grams of silver formed is (moles of silver) x (molar mass of silver).