Question

What is the molar mass of copper (II) nitrate,\[Cu{\left( {N{O_3}} \right)_2}\]?

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. copper (II) nitrate. The molecular or chemical formula of copper (II) nitrate is\[Cu{\left( {N{O_3}} \right)_2}\]. We already know the atomic mass of copper, oxygen and nitrogen which is mentioned below:
$
  Cu = 63.546u \\
  O = 15.9994u \\
  N = 14.0067u \\
$
From the chemical formula, it is clear that copper (II) nitrate comprises of one atom of copper, two atoms of nitrogen and six atoms of oxygen and thus molar mass of this compound can be easily calculated by adding the mass of one copper atom, two nitrogen atoms and six oxygen atom as shown below:
\[
  Molar{\text{ }}mass{\text{ }}of{\text{ Cu}}{(N{O_3})_2} = (1 \times Cu) + (2 \times N) + (6 \times O) \\
   = (1 \times 63.546) + (2 \times 14.0067) + (6 \times 15.9994) = 187.5558gmo{l^{ - 1}} \\
\]
Hence, the molar mass of copper (II) nitrate, \[Cu{\left( {N{O_3}} \right)_2}\] is 187.5558\[gmo{l^{ - 1}}\].

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.