A44.6 mg sample of carbon reacts with sulfur to form 124 mg of the compound. part a what is the empirical formula of the carbon sulfide?

The empirical formula of carbon sulfide = C3S2

calculation

calculate the mass of S used = 124-44.6= 79.4 grams

find the moles of each element

that is carbon(C)= 44.6/12= 3.717 moles    

          sulfur (S) = 79.4/32= 2.48 moles

find the mole ratio by dividing each mole with the smallest mole( 2.48)

that is carbon = 3.717/2.48 = 1.5

        sulfur = 2.48/2.48= 1

multiply by 2 to remove the decimal

= C=1.5 x2=3

S= 1/2 =2

therefore the empirical formula = C3S2

V=d/t