2282018 1130 PM 4 1015 2202018 0320 PM Gradebook Question 11

2/28/2018 11:30 PM 4 10/15 2/20/2018 03:20 PM Gradebook Question 11 of 15 Map General Chemistry 4th Edition University Science Books Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is K, 9.40 at 900 K How many grams of CS2(g) can be prepared by heating 10.6 moles of S2(g) with excess carbon in a 6.85 L reaction vessel held at 900 K until equilibrium is attained? Next Ext

Solution

Molarity of S2 = moles/Volume

= 10.6/6.85

= 1.547 M

Reaction with ICE TABLE

S2 + C = CS2

I 1.547

C - x +x

E 1.547-x x

Equilibrium constant expression of the reaction

Kc = [CS2] /[S2]

9.40 = x/(1.547-x)

6.076 - 9.40x = x

x = 0.5842

Molarity of CS2 prepared = 0.5842 mol/L

Moles of CS2 prepared = molarity x volume

= 0.5842 mol/L x 6.85 L

= 4 mol

Mass of CS2 prepared = moles x molecular weight

= 4 mol x 76.139 g/mol

= 304.71 g