# Chem

At 58.8 degrees C and at a total pressure of 1.00 atm the mole percent of acetone in the vapor state above a solution of acetone and water containing 70. mol % acetone is 87.5%. Assuming the solution to obey Raoult's Law, determine the vapor pressure of pure water at this temperature. Comparing your results to the actual value of 141 mmHg, what does this suggest about the acetone-water solution?

I calculated the first part like so:
1.00 atm= .875 * x
1.14 atm= x

I converted 141 mmHg to atm, which turned out to be .186- obviously quite a bit lower than the answer found above. I'm not sure what this says about the mixture, however.

I get a smaller number than 1.14.
Isn't
P(water)/P(total) = X(water) = 0.875.

Then P(total)*X(water) = P(water) = 1*0.875 = 0.875 atm. That's still very much higher than 0.186 atm. Would you think it says the acetone/water mixture is not an ideal solution?
Check my thinking. Check my work.

1. 👍 0
2. 👎 0
3. 👁 135

## Similar Questions

1. ### CHEMISTRY

One mole of H2O(g) at 1.00 atm and 100 degrees C occupies a volume of 30.6 L. When one mole of H2O(g) is condensed to one mole of H2O(l) at 1.00 atm and 100 degrees C, 40.66 kJ of heat is released. If the density of H2O(l) at this

asked by Anonymous on July 14, 2010
2. ### Chemistry-DrBob222

A 1.0 L ball containing Ar at 5 atm is connected to a 10.0 L ball containing N2 at 2atm. A)Calculate the partial pressures and mole fractions of Ar and N2 after the valve is opened and the gases are allowed to mix (they fill the

asked by Student on March 11, 2016
3. ### Chemistry

A 1.0 L ball containing Ar at 5 atm is connected to a 10.0 L ball containing N2 at 2atm. A)Calculate the partial pressures and mole fractions of Ar and N2 after the valve is opened and the gases are allowed to mix (they fill the

asked by Nevaeh on March 12, 2016
4. ### Chemistry-DrBob222

A 1.0 L ball containing Ar at 5 atm is connected to a 10.0 L ball containing N2 at 2atm. A)Calculate the partial pressures and mole fractions of Ar and N2 after the valve is opened and the gases are allowed to mix (they fill the

asked by Nevaeh on March 11, 2016
5. ### Chemistry/Equilibrium calculations

Hi! Thank you so much for your answer! according to my calculations...I got: 1 bar = 750 mm Hg = 0.986 atm. At constant T and P, volume and moles are proportional, so volume percent = mole %. Pa = (xa)(Pt) , , ,the partial

asked by Mary on August 16, 2008
6. ### Chemistry

Two gases are mixed in a 10.0L fixed volume flask: 8.0 L of O2 at 2.00 atm and 2.0 L of N2 at 3.00 atm. A) Calculate the partial pressure for each gas and the total pressure. I got ... PO2 = 1.60 atm PN2= 0.600 atm B) How much

asked by Student on March 8, 2016
7. ### Chemistry

Two gases are mixed in a 10.0L fixed volume flask: 8.0 L of O2 at 2.00 atm and 2.0 L of N2 at 3.00 atm. A) Calculate the partial pressure for each gas and the total pressure. I got ... PO2 = 1.60 atm PN2= 0.600 atm B) How much

asked by Student on March 8, 2016
8. ### Chemistry

In a gas mixture of He, Ne, and Ar with a total pressure of 8.40 atm, the mole fraction of Ar is ________ if the partial pressures of He and Ne are 1.50 and 2.00 atm respectively. pHe = 1.50 atm. pNe = 2.00 atm. pAr = 8.40 atm -

asked by john on January 14, 2007
9. ### Chemistry

A 1.0 L ball containing Ar at 5 atm is connected to a 10.0 L ball containing N2 at 2 atm. a) Calculate the partial pressure and mole fractions of argon and nitrogen after the valve is opened and the gases are allowed to mix (they

asked by Anonymous on January 31, 2016
10. ### Chemistry-DrBob222

Is the answer for part c 0.91? A 1.0 L ball containing Ar at 5 atm is connected to a 10.0 L ball containing N2 at 2atm. A)Calculate the partial pressures and mole fractions of Ar and N2 after the valve is opened and the gases are

asked by Nevaeh on March 14, 2016

More Similar Questions