[Borek]

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?

[sjb]

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  COS + H₂O

CaCl₂  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.

[Rutherford]

I got 3.062*10^-3.

[Borek]

Close, but not perfect.

[Sophia7X]

0.00282?

[Borek]

Raderford was closer.

[Rutherford]

Done more precisely and got that k=3.1507*10^-3.

[Borek]

3.15×10^-3 it is 

Compare E. Terres, H. Wesemann, Angew.Chem. 45, 795 (1932).