Carbon disulfide is prepared by heating sulfur and charcoal

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is

S2(g) + C(s) <=> CS2(g) Kc=9.40 at 900 K

How many grams of CS2(g) can be prepared by heating 19.0 moles of S2(g) with excess carbon in a 9.25 L reaction vessel held at 900 K until equilibrium is attained?

*Hint*Start by finding the initial concentration of S2 using the number of moles and the volume. Then, set up a table of initial and final concentrations, where the change in concentration of the product is designated as x.

Solution

Carbon disulfide is produced industrially by passing sulfur vapors over hot charcoal:

C + 2S = CS2

method of limiting reactant is used that is
2 mole of sulphur produce cs2 = 1mol
one // /// // // // // = 1/2 mol
then 23.3 mole produce =23.3 x 1/2 mole
then apply the formula
mole=mass/molar mass
as u have mole and want to calculate mass so rearrange the above formula
mass=mole x molar mass
molar mass of cs2 = 12+(2x32)
= 12+ 64 = 72