Introduction

Electrolysis is a chemical process that uses an electric current to drive a non-spontaneous chemical reaction. It is often used to determine the atomic masses of elements. In this case, we have a certain metal with a valency of 3, and we need to determine its atomic mass using the information provided.

Given Data
- Current (I) = 0.550 A
- Mass of metal deposited (m) = 0.55 g
- Time (t) = 100 min

Explanation

To determine the atomic mass of the metal, we need to calculate the number of moles of the metal deposited and then divide it by the mass deposited.

1. Calculate the charge passed (Q):
- Q = I * t = 0.550 A * 100 min = 55 C (Coulombs)

2. Calculate the number of moles (n) of electrons transferred:
- Since the valency of the metal is 3, each metal ion requires 3 moles of electrons to be reduced.
- n = Q / (Faraday's constant * valency)
- Faraday's constant (F) = 96485 C/mol
- n = 55 C / (96485 C/mol * 3)
- n ≈ 0.00060 mol

3. Calculate the molar mass (M) of the metal:
- M = m / n
- M = 0.55 g / 0.00060 mol
- M ≈ 917 g/mol

Conclusion

Therefore, the atomic mass of the metal is approximately 917 g/mol. It is important to note that this calculation assumes 100% efficiency and ideal conditions, which may not always be the case in practice. Electrolysis provides a valuable method for determining atomic masses and can be used to study various chemical reactions and elements.

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