Consider a soulution containing liquids A and B where the mole fraction of B is 0.60. Assuming ideality, calculate the mole fraction of A in the vapor at equilibriumwith this solution at 25 degrees C. (the vapor pressures of pure liquid A and B at 25 degrees C are 117.7 torr and 400.0 torr, respectively)

answer

watching

1,346

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Beverley SmithLv2

17 May 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

An ideal solution at 298 K is made up of the volatile liquids A and B, for which the vapor pressures at that temperature (when pure) are PAÂº = 125 Torr and PBÂº = 46.3 Torr. As the pressure is reduced from 450 Torr the first vapor (first bubble) is observed at a pressure of 70.0 Torr. What is the mole fraction of A in the liquid mixture?

A. A solution of hexane and heptane at 30 degrees C with hexane mole fraction 0.305 has a vapor pressure of 95.0 torr and a vapor-phase hexane mole fraction of 0.55. Find the vapor pressures of pure hexane and heptane at 30 degrees C. State any approximations made.

B. At 25 degrees C and 1 atm, a solution of 72.061 g of H2O and 192.252 g of CH3OH has a volume of 307.09 cubic cm. In this solution the partial molar volume of water is 16. 488 cubic cm/mol. Find the partial molar volume of ethanol in this solution.