A compound is found to contain 63.52% iron and 36.48% sulfur. Find its empirical formula.

A compound has 63.52% iron and 36.48% sulfur. I assume
this is the percentage of the mass of the two elements as found in the compound of which
we have to determine the empirical formula.

We know that
the atomic mass of iron is 56 and the atomic mass of sulfur is
32.

Let the empirical formula of the compound be
Fe(x)S(y)

As the mass of the sulfur in the compound and the
mass of the iron in compound is in the ratio 36.48/63.52, we have: 32*y/ 56*x =
36.48/63.52

=> 32y/56x =
36.48/63.52

=> y/x =
(36.48/63.52)*(56/32)

=> y/x =
1

This gives an equal number of sulfur and iron atoms in
the compound.

Therefore the empirical formula
of the compound is FeS.