In: Chemistry
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g)+C(s)↽−−⇀CS2(g)?c=9.40 at 900 K How many grams of CS2(g) can be prepared by heating 15.6 mol S2(g) with excess carbon in a 7.05 L reaction vessel held at 900 K until equilibrium is attained?
mass of CS2(g) :
Balanced reaction is
S2(g) + C(s) ↔ CS2(g)
Initial [S2] = 2.213 M
(molarity = no. of mole / volume in liter
initial molarity of S2 = 15.6 / 7.05 = 2.213 M)
Kc = 9.40
Make ICE table to calculate equilibrium concentration of reactant and product.
Concentration |
S2 (g) |
CS2 (g) |
Initial concentration |
2.213 M |
0 |
Change in concentration |
-X |
+X |
Equilibrium concentration |
2.213 –X |
X |
Kc = [CS2] / [S2]
Substitute value in above equation
9.40 = (X) / (2.213 - X )
(9.40) x (2.213 - X ) = X
20.8022 - 9.40 X = X
20.8022 = X + 9.40 X
10.40 X = 20.8022
X = 20.8022 / 10.40
X = 2
Equilibrium concentration of CS2 = X = 2 M
No. of moles = molarity X volume in liter
moles of CS2 at equilibrium = 2 X 7.05 = 14.10 mole
molar mass of CS2 = 76.139 g/mol
mass of compound in gm = no. of moles X molar mass
Gm of CS2 = 14.10 X 76.139 = 1073.56 gm
Mass of CS2 = 1073.56 gm