54. Solving a chemistry problem
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298. A mol of H2 and a mol of Sb2S3 are introduced into a reaction vessel and heated to 713 K. The equilibrium constant of the reaction
Sb2S3(s) 3H2 → 2Sb(s) 3H2S
at this temperature is 0.429. Determine how many moles of H2 are consumed and how many grams of Sb are formed when equilibrium is reached.
Sb2S3(s) 3H2 → 2Sb(s) 3H2S
at this temperature is 0.429. Determine how many moles of H2 are consumed and how many grams of Sb are formed when equilibrium is reached.
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