How do I find the empirical formula of this compound

An organic compound was found to contain only C, H, and Cl. When a 1.50 g sample of the compound was completely combusted in air, 3.52 g of CO2 was formed. In a separate experiment the chlorine in a 1.10 g sample of the compound was converted to 1.40 g of AgCl.

Molar mass AgCl is 143.32 g mol−1 so 1.40 g of AgCl means 0.01 moles of Chlorine in the 1.10 g of sample, the grams of chlorine would be 0.0355, so 1.10-0.355 = 0.745 g in C an H moles.
assuming mono-chloro compound a good hypo is C6H5Cl
combustion being C6H5Cl + 7O2 ----> 6CO2 + 2H2O + HCl
3.52 g CO2 implying 0.08 moles, so for C6H5Cl we have 0.0133 mol the expected MW is 112.5
and this is very OK with C6H5Cl