What is the empirical formula, did I do this question correctly?

a)
Atomic masses: C = 12.0, H = 1.0, Cl = 35.5

Mole ratio C : H : Cl
= (24.78/12.0) : (2.08/1.0) : (73.14/35.5)
= 2.07 : 2.08 : 2.06
= (2.07/2.06) : (2.08/2.06) : (2.06/2.06)
= 1.00 : 1.01 : 1.00
= 1 : 1 : 1

The empirical formula = CHCl


b)
Let (CHCl)n be the molecular formula.

Molar mass of the compound :
(12.0 + 1.0 + 35.5) n = 193.9
48.5 n = 193.9
n = 4

The molecular formula = C₄H₄Cl₄

It appears that your math is correct. If we take a 100-gram sample of the compound, that's 24.78 grams of carbon (about 2 moles of carbon), 2.08 grams of hydrogen (about 2 moles of hydrogen), and 73.14 grams of chlorine (again, about 2 moles of chlorine). So the C, H, and Cl are in a 1:1:1 mole ratio, which gives the empirical formula CHCl

It appears that your molecular formula calculation is correct as well. One possible quibble: are you meant to write the answer as (CHCl)4, or as C4H4Cl4? Check with your teacher to be sure.

I hope that helps. Good luck!