Question

Sean plated an unknown metal onto his silver earring which initially weighed 1.41 g. He constructs an electrolytic cell using his ring as one of the electrodes. After running the cell, 0.022 moles of the unknown metal was plated onto his ring and the mass of the ring increased to 3.952 g. What is the atomic weight of the unknown metal in g/mol

Answer 1

115 g/mol

Step-by-step explanation:

Step 1: Given data

• Initial mass of the earring (mi): 1.41 g

• Final mass of the earring (mf): 3.952 g

• Moles of the unknown metal deposited (n): 0.022 mol

Step 2: Calculate the mass of the unknown metal deposited

An earring is plated in an electrolytic cell. The mass of the unknown metal deposited can be calculated using the following expression.

m = mf - mi

m = 3.953 g - 1.41 g

m = 2.54 g

Step 3: Calculate the molar mass (M) of the unknown metal

0.022 moles of the metal have a mass of 2.54 g. The molar mass of the metal is:

M = m/n

M = 2.54 g / 0.022 mol

M = 115 g/mol