1) At a pressure of 760 torr, formic acid (HCOOH; boiling point = 100.7 oC) and...

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Chemistry

1) At a pressure of 760 torr, formic acid (HCOOH; boiling point= 100.7 ^oC) and water (H₂O; boiling point =100.0 ^oC) form an azeotropic mixture, boiling at 107.1^oC, that is 77.5% by mass formic acid. At the boilingpoint of the azeotrope (107.1 ^oC), the vapor pressure ofpure formic acid is 917 torr, and that of pure water 974 torr. Ifthe solution obeyed Raoult's law for both components, what would bethe vapor pressure (in torr) of formic acid at 107.1^oC?
2) If the solution obeyed Raoult's law for both components, whatwould be the vapor pressure of the water (in torr) at 107.1^oC?
3) If the solution obeyed Raoult's law for both components, whatwould be the total vapor pressure (in torr) at 107.1^oC?

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4.5 Ratings (809 Votes)

1 let the mixture be 100 g then mass of HCOOH 775 mass of water 225 now we know that moles mass molar mass so moles of HCOOH 775 46 16848 moles of H20 225 18 125 now total moles See Answer

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