Question

When components A and B are mixed, this system has a maximum temperature azerotrope at 1-bar...

When components A and B are mixed, this system has a maximum temperature azerotrope at 1-bar pressure. Suppose 2 moles of pure A is in vapor-liquid equilibrium and 0.1 moles of liquid B is added at constant pressure. What happens? Explain why.

Homework Answers

Answer #1

When mixture solution shows negative deviation from Roult's law and forms maximum boiling azetrope (boiling point higher than either of the components)

For this case when 2 mol of A in vapor liquid equilibrium mixed with 0.1 mol of B the interaction between molecule of A and B which mean A-B bond will be stronger than A-A bond or B-B bond. As a result of strong A-B interaction total vapor pressure of resultant mixture will be less than what we calculate from Roult's law hence shows negative deviation and forms maximum boiling azeotrope. Also total volume of mixture less than sum of individual volume of A and B.

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 equal amounts (in moles) of liquid components A and B. The vapor pressure...
A solution contains equal amounts (in moles) of liquid components A and B. The vapor pressure of pure A is 100 mmHg and that of pure B is 200 mmHg. What is the vapor pressure above the solution assuming it is an ideal solution? The experimentally measured vapor pressure is 150 mmHg. What does this indicate about relative strengths of the interactions between solute and solvent molecules?   Please help me
The reversible, gas-phase reaction, 2A->B is in equilibrium in a piston-cylinder at 3.5-bar pressure. At equilibrium,...
The reversible, gas-phase reaction, 2A->B is in equilibrium in a piston-cylinder at 3.5-bar pressure. At equilibrium, the system contains 2.0 mol A and 3.0 mol B. When 5.0 mol of an inert gas are added to the system, how many moles of B are present at equilibrium? The pressure and temperature do not change. Assume ideal gases.
For a liquid, does entropy increase, decrease, or stay about the same if: 1) Pressure increases...
For a liquid, does entropy increase, decrease, or stay about the same if: 1) Pressure increases isothermally 2)Temperature increases isobarically? 3)Two pure liquid species are mixed at constant temperature? 4)The liquid evaporates at the vapor pressure? 5)The liquid freezes at the melting temperature?
A liquid mixture of two unknown liquids, A and B, has a total vapor pressure of...
A liquid mixture of two unknown liquids, A and B, has a total vapor pressure of 0.04 bar. The vapor pressure of pure A under the same conditions is 0.03 bar, and the vapor pressure of pure B under the same conditions is 0.05 bar. Using Raoult’s Law, what are the mole fractions of A and B in solution?
Thermodynamics: Consider the equilibrium reaction A(g) + B(g) -><- C(g)+D(g). At T=298 K, the standard enthalpies...
Thermodynamics: Consider the equilibrium reaction A(g) + B(g) -><- C(g)+D(g). At T=298 K, the standard enthalpies of formation of the components in the gas phase are -20, -40, -30, and -10 kJ/mol for A,B,C, and D, respectively. The standard-state entropies of the components in the gas phase are 30, 50, 50, and 80 J/(mol K), in the same order. The vapor pressure of liquid C at this temperature is 0.1 bar, while all other components are volatile gases with Henry's...
1. The reaction I2(g) + Cl2(g) ⇔ 2 ICl(g) is at equilibrium when the partial pressures...
1. The reaction I2(g) + Cl2(g) ⇔ 2 ICl(g) is at equilibrium when the partial pressures are: I2 = 0.027 atm, Cl2 = 0.027 atm and ICl = 0.246 atm. The partial pressure of ICl is then increased to 0.500 atm by adding ICl. a. When the system re-establishes equilibrium, what is the partial pressure of Cl2(g)? b. When the system re-establishes equilibrium, what is the partial pressure of ICl(g) c. When the system re-establishes equilibrium, what is the partial...
. A closed, nonreactive system contains species 1 and 2 in vapor/liquid equilibrium. Species 2 is...
. A closed, nonreactive system contains species 1 and 2 in vapor/liquid equilibrium. Species 2 is a very light gas, essentially insoluble in the liquid phase. The vapor phase contains both species 1 and 2. Some additional moles of species 2 are added to the system, which is then restored to its initial T and P. As a result of the process, does the total number of moles of liquid increase, decreases, or remain unchanged? Please consider the question using...
Pure hexane (C6) exists as V + L as shown. Pure heptane (C7) liquid is injected...
Pure hexane (C6) exists as V + L as shown. Pure heptane (C7) liquid is injected into the vapor at constant temperature and pressure. After injection the overall mixture is 10 mol% C7. What happens (circle the best answer)? (a) All the C7 goes to L and the V is only C6. (b) The vapor is mostly C6 with some C7. (c) All the vapor condenses. (d) All the liquid evaporates. (e) None of the above. Explain
The reaction ?2?12 (g) ⇆ ?4?6(g) + ?2?6(g) is at equilibrium at 1 bar at 700...
The reaction ?2?12 (g) ⇆ ?4?6(g) + ?2?6(g) is at equilibrium at 1 bar at 700 K. You may assume that there are no competing reactions when cyclohexane (C6H12) is heated to 700 K, and you may treat all gases as ideal (perfect) gases. (a) Write an expression for the equilibrium constant, K, in terms of partial pressures. State the units of pressure in your expression. (b) The partial pressure of each gas was measured for the above reaction at...
1. Find values of residual enthalpy for ethylene at 400 K and 25 bar using Peng-Robinson...
1. Find values of residual enthalpy for ethylene at 400 K and 25 bar using Peng-Robinson equation of state. 2. Find values of residual Gibbs energy, enthalpy and entropy for n-heptane at 500 K and 100 bar using Virial equation of state. 3. Estimate the values of Compressibility factor, enthalpy and entropy for Benzene and cyclohexane if it compressed from 650 K and 60 bar to 500 K and 110 bar. 4. Calculate ΔU and ΔH for 1 kg of...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT