Problem: 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 13.0 moles of S2 (g) with excess carbon in a 5.85L reaction vessel held at 900 K until equilibrium is attained?

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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 13.0 moles of S2 (g) with excess carbon in a 5.85L reaction vessel held at 900 K until equilibrium is attained?

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