Question

A solution that contains nitromethane (1) in acetonitrile (2) is heated at a constant pressure of...

A solution that contains nitromethane (1) in acetonitrile (2) is heated at a constant pressure of 1 bar until the first bubble appears. If the temperature of the solution at this point is 85C, what is the composition of the original solution?

You may assume that the solution is ideal. The saturation pressures for the pure components (in kPa) for T in C are given by

ln(p1sat) = 14.2742 – 2945.47/(224 + T)

ln(p2sat) = 14.2043 – 2972.64/(209 + T)

Homework Answers

Answer #1

Apply Raoults law:

x1*P°1 = y1*PT

x2*P°2 = y2*PT

and

ln(P°1) = 14.2742 – 2945.47/(224 + T)

ln(P2°) = 14.2043 – 2972.64/(209 + T)

x2 = 1-x1

y2 = 1-y1

then..

if P = 1 bar --> 100 kPa

T = 85°C

substitute

ln(P°1) = 14.2742 – 2945.47/(224 + 85) = 4.74193 kPa

ln(P2°) = 14.2043 – 2972.64/(209 + 85) = 4.09327 kPa

x1*P°1 = y1*PT

x2*P°2 = y2*PT

Pt = 100 kPa

x1*4.74193 = y1*100

x2*4.09327 = y2*100

subs

x1*4.74193 = y1*100

(1-x1)*4.09327 = (1-y1)*100

x1 = 100/4.74193*y1 = 21.088*y1

(1- 21.088*y1)*4.09327 = (1-y1)*100

4.09327 - 21.088*4.09327 y1 = 100 - 100y1

y1(21.088*4.09327 +100) = 100-4.09327

y1 = 95.9067/186.318 = 0.51474

y2 = 1-0.51474 = 0.48526

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A solution contains 50.0 g of heptane (C7H16) and 50.0g of octane (C8H20) at 25oC. The...
A solution contains 50.0 g of heptane (C7H16) and 50.0g of octane (C8H20) at 25oC. The vapor pressures of pure heptane and pure octane at this temperature are 45.8 and 10.9 Torr, respectively. Assuming ideal behavior, calculate the: 1) vapor pressure of each of the solution components in the mixture 2) total pressure above the solution 3) composition of the vapor in mass percent Please explain! Thank you.
We have a mixture, which is an ideal solution in the liquid phase and an ideal-gas...
We have a mixture, which is an ideal solution in the liquid phase and an ideal-gas mixture in the vapor phase, of n-heptane (1) and n-octane (2) at a pressure of 1 bar with z1 = 0.25. (a) What are the bubble and dew temperatures? (b) Calculate the heat required to bring the solution from its bubble temperature to its dew temperature. Please use the Antoine equations given in P11.5 to find the saturation pressures of these species. lnPsat= A-B/(C+t)...
The system acetone(1)/acetonitrile(2)/nitromethane(3) at 80oC(353.15K) and 110kPa has the overall composition, z1=0.45, z2=0.35, z3=0.20. Assuming that...
The system acetone(1)/acetonitrile(2)/nitromethane(3) at 80oC(353.15K) and 110kPa has the overall composition, z1=0.45, z2=0.35, z3=0.20. Assuming that Raoult's law is appropriate to this system, determine L,V. The vapor pressures of the pure species at 80oC( 353.15K) are: P1(sat)=195.75, P2(sat)=97.84, P3(sat)=50.32kPa. Note: L is the moles of liquid with mole fraction xi , V is the moles of vapor, with mole fraction yi Can you help me to figure out V? I have done this problem until the whole bunch equation of...
A solution contains 49.0 g of heptane (C7H16)and 59.0 g of octane (C8H18) at 25 ∘C....
A solution contains 49.0 g of heptane (C7H16)and 59.0 g of octane (C8H18) at 25 ∘C. The vapor pressures of pure heptane and pure octane at 25 ∘C are 45.8 torr and 10.9 torr, respectively. Assuming ideal behavior, calculate each of the following. (Note that the mole fraction of an individual gas component in an ideal gas mixture can be expressed in terms of the component's partial pressure.) A) The vapor pressure of heptane in the mixture B) The Vapor...
Please show all work. Thanks! Consider a solution with xA = 0.220 at 30?C in equilibrium...
Please show all work. Thanks! Consider a solution with xA = 0.220 at 30?C in equilibrium with the vapor. The vapor pressures of the pure components at this temperature are: p? A = 73.0kPa and p? B = 92.1kPa. (a) Predict the vapor pressure and its composition at these conditions assuming ideal solution. (b) Experimentally it was found that the actual vapor pressure was 1.00atm and yA = 0.314. Calculate the activities and activity coe?cients of both components in this...
Air with a mass of 2 kg is heated at a constant pressure of 200 kPa...
Air with a mass of 2 kg is heated at a constant pressure of 200 kPa to a temperature of 500°C. Calculate the entropy change if the initial volume is 0.8 m3. Take ???? = 1.00 kJ/kg ? K and model air as an ideal gas. (Hint: Use the appropriate TdS [Gibbs] relation to calculate entropy change.)
One more of an ideal gas initially at 27oC and 1 bar pressure is heated and...
One more of an ideal gas initially at 27oC and 1 bar pressure is heated and allowed to expand reversibly at a constant pressure until the final temperature is 327oC. For this gas, Cv,m = 2.5R, constant over the temperature range. (Note from SRB: Cv,m is the molar heat capacity. An earlier version of the 5th edition that I used last year used Cv with a bar over it, as we have been doing in class. Sorry for any confusion.)....
1- Acetone (1) and Methanol (2) form an azeotrope boiling at 55.7oC at 1 atm pressure,...
1- Acetone (1) and Methanol (2) form an azeotrope boiling at 55.7oC at 1 atm pressure, with a composition x1 = 0.80. Calculate the van Laar Coefficients for the system. 2- Perry (Table 13-1) quotes the following x,y,T data for Acetone (1) and Methanol (2) at 101.3 kPa total pressure. Estimate the van Laar constants A12 & A21. T/oC 64.65 61.78 59.60 58.14 56.96 56.22 55.78 55.41 55.29 55.37 55.54 55.92 56.21 x1 0 0.091 0.190 0.288 0.401 0.501 0.579...
A Microscale Approach to Organic Laboratory Techniques (5th Edition), CH 15, #1. d. e. ONLY. PLEASE...
A Microscale Approach to Organic Laboratory Techniques (5th Edition), CH 15, #1. d. e. ONLY. PLEASE given: In the accompanying chart are appropriate vapor pressures for benzene and toluene at various temperatures: Temp (C) mmHg Temp (C) mmHg Benzene 30 120 Toluene 30 37 40 180 40 60 50 270 50 95 60 390 60 140 70 550 70 200 80 760 80 290 90 1010 90 405 100 1340 100 560 110 760 1.a. What is the mole fraction...
1) Use Henry's law to determine the molar solubility of helium at a pressure of 1.9...
1) Use Henry's law to determine the molar solubility of helium at a pressure of 1.9 atm and 25 ∘C. Henry’s law constant for helium gas in water at 25 ∘C is 3.70⋅10−4M/atm. 2) A 2.800×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.2 mL...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT