<u>Answer:</u> The molecular formula of the compound is 
<u>Explanation:</u>
The molecular formula is the chemical formula that tells about the number of atoms of each element present in a compound. Molecular formula and empirical formula can also be the same when the number of atoms is in the simplest whole-number ratio.
To calculate the molecular formula, the number of atoms of the empirical formula is multiplied by a factor known as valency that is represented by the symbol, 'n'.
...(1)
Given empirical formula is 
Empirical mass = ![[(1\times 30.97) + (3\times 15.99)]=78.94 g/mol](https://tex.z-dn.net/?f=%5B%281%5Ctimes%2030.97%29%20%2B%20%283%5Ctimes%2015.99%29%5D%3D78.94%20g%2Fmol)
Molecular mass = 157.9 g/mol
Plugging values in equation 1:

Molecular formula of the compound becomes 
Hence, the molecular formula of the compound is