Question

How many moles are present in 165 g of Manganese?

Answer 1

Hint: To solve this question, we first need to understand what is a mole. Mole is the SI unit of measurement and is used to determine the amount of a substance. A mole of any substance has exactly $6.022\times {{10}^{23}}$ particles which can be ions, atoms, electrons, or molecules.

Complete step by step answer:
We know that if one mole of a substance is present, it has exactly the Avogadro number $({{N}_{A}})$ of particles.
${{N}_{A}}=6.022\times {{10}^{23}}$
Now, the mass of a sample can be given by the sum of the mass of all the particles in it.
So, we can say that the mass of one mole of a compound is equivalent to the mass of all the particles contained in one mole of a substance i.e., $6.022\times {{10}^{23}}$ particles.
The mass of one mole of a substance is known as the molar mass of that substance. Its SI base unit is kg/mol but it is usually expressed in g/mol. It is a bulk property of a substance, not a molecular property.
Now, the molar mass of a sample is given by the mass of the sample substance divided by the number of moles of the substance present in the sample.
\[M=\dfrac{m}{n}\]
So, the number of moles in a given sample can be given by
\[n=\dfrac{m}{M}\]
Where n is the number of moles,
m is the mass of the substance given (in grams), and
M is the molar mass of the substance (in g/mol).
We know that the molar mass of Manganese (Mn) is 54.938 g/mol.
It is given to us that the mass of the sample substance is 165 grams.
So, the number of moles of the substance in the sample is
\[
   n=\dfrac{165g}{54.938g/mol} \\
  n\cong 3.003mol \\
\]
Hence there are approximately 3.003 moles in a sample of 165 grams of Manganese (Mn).

Note: It must be noted that in 2019, the SI base unit of molar mass was redefined. According to the new definition, the molar mass constant is
\[{{M}_{u}}=0.99999999965\times {{10}^{-3}}kg/mol\]
And not $1\times {{10}^{-3}}kg/mol$.
But since the change is so insignificant, for practical purposes, the molar mass of an element is still considered to be equivalent to the atomic mass of the element.