Question

What is the molar mass of ammonium sulfate?

Answer 1

Hint : The molar mass of any chemical compound refers to the ratio of mass of a sample of that particular compound and the amount of substance in that particular sample (in moles). The molar mass is actually a bulk characteristic of a substance rather than molecular. The molar mass is generally represented as $gmo{l^{ - 1}}$ .

Complete Step By Step Answer:
The molar mass of any compound can be found out by adding the relative atomic masses of each element present in that particular compound. The number of atoms in a compound can be determined from their chemical formula.
Now, let us calculate the molar mass of the given compound i.e. ammonium sulfate. The chemical formula of ammonium sulfate is ${(N{H_4})_2}S{O_4}$ while its structure is depicted below:

We already know the atomic mass of nitrogen, hydrogen, sulfur and oxygen which is mentioned below:
N = 14.0067u \\\ H = 1.00784u \\\ S = 32.065u \\\ O = 15.9994u \\\
From the chemical formula and structure, it is clear that ammonium sulfate comprises of two atoms of nitrogen, eight atoms of hydrogen, one atom of sulfur and four atoms of oxygen and thus molar mass of this compound can be easily calculated by adding the mass of two nitrogen atoms, eight hydrogen atoms, one sulphur atom and four oxygen atom as shown below:
Molar{\text{ }}mass{\text{ }}of{\text{ }}{(N{H_4})_2}S{O_4} = (2 \times N) + (8 \times H) + (1 \times S) + (4 \times O) \\\ = (2 \times 14.0067) + (8 \times 1.00784) + (1 \times 32.065) + (4 \times 15.9994) = 132.13872gmo{l^{ - 1}} \\\
Hence, the molar mass of ${(N{H_4})_2}S{O_4}$ is 132.13872 $gmo{l^{ - 1}}$ .

Note :
Molar mass plays a significant role in chemistry especially during setting up an experiment. During testing principles which involve specific amounts or quantities of a substance, molar mass is used to figure out the exact quantity to be weighed of that particular substance. Basically molar mass is used to determine the stoichiometry in the chemical reactions as well as equations.