The vapor pressures of each component in a mixture of propanone (acetone, A) and trichloromethane (chloroform, C) were measured at 35°C with the following results:In the above, xC is molar fraction of compound C.Check whether the mixture conforms to Raoult’s law for the component in large excess and to Henry’s law for the minor component.Provide relevant graphs with calculations.Find the Henry’s law constant for each of the two substances.If the substantial difficulties are encountered in finding the Henry’s law constants, explain what these problems are and why they occur. ### Data Table TranscriptionThis table presents a set of data that includes the mole fraction of a component \( x_C \), and corresponding partial pressures \( p_C \) and \( p_A \), both measured in kilopascals (kPa).| \( x_C \) | \( p_C \) (kPa) | \( p_A \) (kPa) ||-----------|----------------|----------------|| 0 | 0 | 46.3 || 0.20 | 4.7 | 33.3 || 0.40 | 11 | 23.3 || 0.60 | 18.9 | 12.3 || 0.80 | 26.7 | 4.9 || 1 | 36.4 | 0 |### Explanation- **\( x_C \)**: Represents the mole fraction of component C in the mixture, ranging from 0 to 1.- **\( p_C \) (kPa)**: Shows the partial pressure of component C in kilopascals, increasing as the mole fraction of C increases.- **\( p_A \) (kPa)**: Displays the partial pressure of component A in kilopascals, which decreases as the mole fraction of component C increases.The table illustrates the relationship between the mole fraction of component C and the partial pressures of components C and A, likely representing an experimental or theoretical scenario involving a binary mixture.

Raoult's law will be tested by comparing. Data with straight line for p = xp*. Henry law will be tested by comparing data plotted with the straight line for p=xk. Both Raoults and Henry's law are statements about the form of graph of partial vapour pressure against mole fraction.pj = Xj Pj* ( for each component in the region in which it is in excess) PJ = XJ Kj (Tangent to each partial. vapour pressure at low x, where 1 the component can be treated as the solute.

Answered: The vapor pressures of each component…

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...

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The vapor pressures of each component in a mixture of propanone (acetone, A) and trichloromethane (chloroform, C) were measured at 35°C with the following results: In the above, xC is molar fraction of compound C. Check whether the mixture conforms to Raoult’s law for the component in large excess and to Henry’s law for the minor component. Provide relevant graphs with calculations. Find the Henry’s law constant for each of the two substances. If the substantial difficulties are encountered in finding the Henry’s law constants, explain what these problems are and why they occur.

### Data Table Transcription

This table presents a set of data that includes the mole fraction of a component \( x_C \), and corresponding partial pressures \( p_C \) and \( p_A \), both measured in kilopascals (kPa).

| \( x_C \) | \( p_C \) (kPa) | \( p_A \) (kPa) |
|-----------|----------------|----------------|
| 0 | 0 | 46.3 |
| 0.20 | 4.7 | 33.3 |
| 0.40 | 11 | 23.3 |
| 0.60 | 18.9 | 12.3 |
| 0.80 | 26.7 | 4.9 |
| 1 | 36.4 | 0 |

### Explanation

- **\( x_C \)**: Represents the mole fraction of component C in the mixture, ranging from 0 to 1.
- **\( p_C \) (kPa)**: Shows the partial pressure of component C in kilopascals, increasing as the mole fraction of C increases.
- **\( p_A \) (kPa)**: Displays the partial pressure of component A in kilopascals, which decreases as the mole fraction of component C increases.

The table illustrates the relationship between the mole fraction of component C and the partial pressures of components C and A, likely representing an experimental or theoretical scenario involving a binary mixture.

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