Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equati
ID: 709855 • Letter: C
Question
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.
Explanation / Answer
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