Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equati
ID: 827472 • 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 900K.How many grams of CS2(g) can be prepared by heating 10.9 moles of S2(g) with excess carbon in a 5.80 L reaction vessel held at 900 K until equilibrium is attained?
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s)= CS2(g). KC=9.40 at 900K.
How many grams of CS2(g) can be prepared by heating 10.9 moles of S2(g) with excess carbon in a 5.80 L reaction vessel held at 900 K until equilibrium is attained?
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s)= CS2(g). KC=9.40 at 900K.
How many grams of CS2(g) can be prepared by heating 10.9 moles of S2(g) with excess carbon in a 5.80 L reaction vessel held at 900 K until equilibrium is attained?
How many grams of CS2(g) can be prepared by heating 10.9 moles of S2(g) with excess carbon in a 5.80 L reaction vessel held at 900 K until equilibrium is attained?
How many grams of CS2(g) can be prepared by heating 10.9 moles of S2(g) with excess carbon in a 5.80 L reaction vessel held at 900 K until equilibrium is attained?
Explanation / Answer
S2(g) + C(s)= CS2(g). KC=9.40
10.9 -
10.9 -x x x
Kc = x/(10.9 -x)
9.4 =x/(10.9 -x)
x = 9.8519230769230769 moles
so moles of CS2(g) produced = 9.8519230769230769 moles
grams of CS2(g) = moles * molar mass = 9.8519230769230769 * 76 = 748.7461538461538444 gms