Question

A mixture of 60.0 g of S and 1.02×102 g of Cl2 reacts completely to form S2Cl2 and SCl2. Find the mass of S2Cl2 formed.

Answer 1

the reaction is

3S + 2Cl2 --> S2Cl2 + SCl2

we know that

moles = mass / molar mass

so

moles of S = 60 / 32 = 1.875

moles of Cl2 = 102 / 71 = 1.437

now

from the reaction

moles of S required = 1.5 x moles of Cl2

moles of S required = 1.5 x 1.437 = 2.155

but

only 1.875 moles of S is present

so

S is the limiting reagent

now

moles of S2Cl2 formed = (1/3) x moles of S

= 1.875 / 3

= 0.625

now

mass = moles x molar mass

soo

mass of S2Cl2 formed = 0.625 x 135

mass of S2Cl2 formed = 84.375

so

84.375 grams of S2Cl2 is formed