Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Problem of the Week Archive => Topic started by: Borek on May 21, 2012, 06:19:57 AM
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Another (simple) one taken from the old publication:
Gaseous mixture contained 51.3% (v/v) of H2S, the rest was CO2. 1750 mL of the mixture (measured at 760 mm Hg and 21 °C) was heated to 350 °C, cooled, and pumped through a CaCl2, increasing its mass by 34.7 mg. What is the equilibrium constant of the carbonyl sulfide synthesis from H2S and CO2 at 350 °C?
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Another (simple) one taken from the old publication:
Gaseous mixture contained 51.3% (v/v) of H2S, the rest was CO2. 1750 mL of the mixture (measured at 760 mm Hg and 21 °C) was heated to 350 °C, cooled, and pumped through a CaCl2, increasing its mass by 34.7 mg. What is the equilibrium constant of the carbonyl sulfide synthesis from H2S and CO2 at 350 °C?
OK, here's a start
CO2 + H2S ::equil:: COS + H2O
CaCl2 :rarrow: CaCl2.6H2O (not sure of the exact formula of the hydrate, could be di, or tetra? May be irrelevant)
34.7 mg increase in the weight of CaCl2, means (34.7 x 10-3/18.02) mol of water.
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I got 3.062*10-3.
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Close, but not perfect.
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0.00282?
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Raderford was closer.
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Done more precisely and got that k=3.1507*10-3.
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3.15×10-3 it is :)
Compare E. Terres, H. Wesemann, Angew.Chem. 45, 795 (1932).