**Section 9.11****P9.27** G. Ratcliffe and K. Chao [*Canadian Journal of Chemical Engineering* 47 (1969), 148] obtained the following tabulated results for the variation of the total pressure above a solution of isopropanol \((P_1^* = 1008 \text{ Torr})\) and *n*-decane \((P_2^* = 48.3 \text{ Torr})\) as a function of the mole fraction of the *n*-decane in the solution and vapor phases. Using these data, calculate the activity coefficients for both components using a Raoult’s law standard state.| \(P\) (Torr) | \(x_2\) | \(y_2\) ||--------------|---------|---------|| 942.6 | 0.1312 | 0.0243 || 909.6 | 0.2040 | 0.0300 || 883.3 | 0.2714 | 0.0342 || 868.4 | 0.3360 | 0.0362 || 830.2 | 0.4425 | 0.0411 || 786.8 | 0.5578 | 0.0451 || 758.7 | 0.6036 | 0.0489 |Explanation: The table presents the total pressure data (\(P\) in Torr) as it relates to the mole fraction of *n*-decane in the liquid phase (\(x_2\)) and vapor phase (\(y_2\)). These values are used to determine the activity coefficients, crucial for understanding the deviation of real solutions from ideal behavior under Raoult’s law.

Given as, isopropanol= 1008 Torr, n-decane= 48.3 Torr.

Answered: variation of the total pressur 1 (P¡ =…

Science

Chemistry

variation of the total pressur 1 (P¡ = 1008 Torr) and n-de nction of the mole fraction

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: How many molecules of O2 are contained in a 10.0L tank at 7.53atm and 485k?

A: According to ideal gas equation, ratio of product of pressure and volume to the product of number of…

Q: The pressure of a mixture of nitrogen, carbon dioxide, and oxygen is 190 kPa. What is the partial…

Q: (a) The pressure of the gas if 0.145 mol occupies 237 mL at 25°C. atm (b) The temperature (in…

A: From ideal gas equation - PV = nRT Where - P = pressure V = volume n = number of moles R =…

Q: A gas mixture consists of 320 mg of CH4, 175mg of Ar and 225 mg of Ne. The partial pressure of Ne at…

A: The ideal gas equation is PV =nRTUsing the equation we can calculate volume of the container.…

Q: The gas in the discharge cell of a laser contains (in mole percent) 11% CO2, 5.3% N2, and 84% He.…

A: We know density can be calculated using the formula - DRT=PM Where D=Density(g/L)…

Q: You fill a rigid steel container with a volume of 20 L with nitrogen gas to a pressure of 2000 kpa…

Q: The mole fraction of neon in dry air near sea level is 0.00001818, where the molar mass of neon is…

A: Step 1: Use the Raoult's Law to solve the problem. Refer to the solution below.

Q: What is the mole fraction of Ne in a mixture of gas where the PHe = 64 torr, PNe= 56 torr, Par= 175…

A: The mole fraction of a component in the mixture is defined by the ratio of moles of that substance…

Q: A gaseous mixture contains 422.0 Torr H2(g), 363.7 Torr N2(g), and 89.1 Torr Ar(g). Calculate the…

A: The mole fraction of a component in the mixture is defined as the ratio of moles of that substance…

Q: If nitrogen gas and oxygen gas are combined in a tank, they will be at the same tem perature and…

A: In the kinetic theory of gas, we know the pressure is caused due to collision of the gas molecule on…

Q: A student has a 2.20 L bottle that contains a mixture of O2 , N2 , and CO2 with a total pressure of…

A: Dalton's law of partial pressures :- According this , the total pressure of a mixture of non…

Q: The following reaction was carried out in a 3.00 reaction vessel at 1100 K: C(s) + H₂O(g) = CO(g) +…

A: The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical…

Q: The decomposition of sulfuryl chloride at 320 degrees Celsius proceeds according to a reaction of…

Q: A 515 mL sample of gas is collected at a temperature of 22.0°C and is kept at 122 kPa. The volume…

Q: A gas sample is under an initial set of conditions (i) and is then changed to a final set of…

Q: A gas mixture contains 2.01 mol F, and 1.85 mol CH with a total pressure of 150. kPa. What is the…

A: We have given that Total pressure of gas mixture =PT = 150Kpa Mole of F2 = 2.01mole Mole of CH4 =…

Q: Calculate the delta Ssystem when the state of 2.00 mol of gas molecules, for which Cpm=7/2R, is…

A: The order of randomness of any system is called its entropy. It is a unique property of…

Q: Dalton's law states that the total pressure, Ptotal of a mixture of gases in a container equals the…

Q: A mixture of ideal gases having a total mass of 35 g is placed in a 13 L vessel at 269.0 K. The…

Q: In the combustion of butane at 105 kPa and 292 K 2C4H10(g) + 13O2(g) --> 10H2O(g) + 8CO2(g) What…

A: Given: Pressure of butane is 105 kPa Temperature is 292 K Mass of oxygen is 350 g Volume of butane…

Q: Sketch three isochores for the same gas at three different volumes V1, V2 and V3 where V1 = V3 and…

A: A question based on chemical thermodynamics that is to be accomplished.

Q: 2) Explain the origin of the "a" term in the van der Waals equation. Which has the lower "a"…

Q: Determine the mole fraction of toluene

Q: Dalton's Law of Partial Pressures states that the total pressure of a gas mixture is equal to the…

A: Dalton’s Law (also called Dalton’s Law of Partial Pressures) states that the total pressure exerted…

Question

**Section 9.11**

**P9.27** G. Ratcliffe and K. Chao [*Canadian Journal of Chemical Engineering* 47 (1969), 148] obtained the following tabulated results for the variation of the total pressure above a solution of isopropanol \((P_1^* = 1008 \text{ Torr})\) and *n*-decane \((P_2^* = 48.3 \text{ Torr})\) as a function of the mole fraction of the *n*-decane in the solution and vapor phases. Using these data, calculate the activity coefficients for both components using a Raoult’s law standard state.

| \(P\) (Torr) | \(x_2\) | \(y_2\) |
|--------------|---------|---------|
| 942.6 | 0.1312 | 0.0243 |
| 909.6 | 0.2040 | 0.0300 |
| 883.3 | 0.2714 | 0.0342 |
| 868.4 | 0.3360 | 0.0362 |
| 830.2 | 0.4425 | 0.0411 |
| 786.8 | 0.5578 | 0.0451 |
| 758.7 | 0.6036 | 0.0489 |

Explanation: The table presents the total pressure data (\(P\) in Torr) as it relates to the mole fraction of *n*-decane in the liquid phase (\(x_2\)) and vapor phase (\(y_2\)). These values are used to determine the activity coefficients, crucial for understanding the deviation of real solutions from ideal behavior under Raoult’s law.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 14 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A sample of gas contains (among other things): 7.0% CO, 15% CO2, 4.0% O2 and 4.5%CH4, all by volume. What is the mole fraction of methane in the sample?
Calculate the partial pressure of propane (C3H8) in a mixture that contains equal masses of propane and butane (C4H10) at 50°C and 764 Torr.
I need help with 15.37
To determine the molar mass of an unknown gas, its effusion time was compared to Oscon gas, which has a molar mass of 42.005g - mol-1. Asample of Oscon was found to effuse from a container in 41.71 Part A seconds. The same amount of the unknown gas requires 91.76 seconds. Rateoscon Rateunknown Determine the ratio Hint the times are not the individual rates themselves. Rates are an amount per time. Express your answer using four significant figures. ? RateOncon Rateunknown
A student has a 2.97 L bottle that contains a mixture of O2 , N2 , and CO2 with a total pressure of 4.70 bar at 298 K . She knows that the mixture contains 0.277 mol N2 and that the partial pressure of CO2 is 0.336 bar . Calculate the partial pressure of O2 .
A gas mixture contains 14.8 mol of Br2 and 66.5 mol of F2.(a) Compute the mole fraction of Br2 in the mixture.XBr2 = (b) The mixture is then heated, and the Br2 starts to react with the F2 to give BrF5: Br2(g) + 5F2(g) -> 2BrF5(g) At a certain point in the reaction, 7.70 mol of BrF5 is present. Determine the mole fraction of Br2 in the new mixture. XBr2 =
Ne(g)Ne(g) effuses at a rate that is ______ times that of Xe(g)Xe(g) under the same conditions.