Question

Q 3. 94 Disulfide dichloride (S2Cl2) is used in the vulcanization of rubber, a process that prevents the slippage of rubber molecules past one another when stretched. It is prepared by heating sulfur in an atmosphere of chlorine: S8 (l) + 4Cl2(g) 4S2Cl2(l) What is the theoretical yield of S2Cl2 in grams when 4.06 g of S8 are heated with 6.24 g of Cl2? If the actual yield of S2Cl2 is 6.55 g, what is the percent yield?

Answer 1

Now we will calculate the moles of S2Cl2 formed assuming complete reaction for each reactant.

From the reactant S8

4.06 × 4molS2Cl2/1molS8

4.04×4×135.04S2Cl2/256.56gS8

= 0.0633 mol S2Cl2

From the reactant : Cl2

6.24 × 135.04S2Cl2/4×35.5g Cl2

= 0.0880 mol S2CL2