Problem: Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation isS2(g) + C(s) → CS2(g)          Kc = 9.40 at 900 KHow many grams of CS2(g) can be prepared by heating 11.1 moles of S2(g) with excess carbon in a 7.00 L 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 11.1 moles of S2(g) with excess carbon in a 7.00 L reaction vessel held at 900 K until equilibrium is attained?

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