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?Acetone \(\left(\mathrm{H}_{3} \mathrm{CCOCH}_{3}\right)\) has a boiling point of \(56^{\circ} \mathrm{C}\). Based on the data given in Figure 11.25,

Chemistry: The Central Science | 14th Edition | ISBN: 9780134414232 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus ISBN: 9780134414232 1274

Solution for problem 11.50 Chapter 11

Chemistry: The Central Science | 14th Edition

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Chemistry: The Central Science | 14th Edition | ISBN: 9780134414232 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus

Chemistry: The Central Science | 14th Edition

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Problem 11.50

Acetone \(\left(\mathrm{H}_{3} \mathrm{CCOCH}_{3}\right)\) has a boiling point of \(56^{\circ} \mathrm{C}\). Based on the data given in Figure 11.25, would you expect acetone to have a higher or lower vapor pressure than ethanol at \(25^{\circ} \mathrm{C}\)?

Text Transcription:

(H_3CCOCH_3)

56^{\circ} C

25^{\circ} C

Step-by-Step Solution:

Step 1 of 5) Collision frequency increases with temperature, A also has some temperature dependence, but this dependence is much smaller than the exponential term. Therefore, A is considered to be approximately constant. We can calculate the activation energy for a reaction by manipulating the Arrhenius equation. Taking the natural log of both sides of Equation 14.21, we obtain which has the form of the equation for a straight line. A graph of ln k versus is a line with a slope equal to and a y-intercept equal to ln A. Thus, the activation energy can be determined by measuring k at a series of temperatures, graphing ln k versus, and calculating Ea from the slope of the resultant line. We can also use Equation 14.22 to evaluate Ea in a non graphical way if we know the rate constant of a reaction at two or more temperatures. For example, suppose that at two different temperatures T1 and T2 a reaction has rate constants k1 and k2.

Step 2 of 2

Chapter 11, Problem 11.50 is Solved
Textbook: Chemistry: The Central Science
Edition: 14
Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
ISBN: 9780134414232

This full solution covers the following key subjects: . This expansive textbook survival guide covers 29 chapters, and 2820 solutions. The answer to ā€œ?Acetone \(\left(\mathrm{H}_{3} \mathrm{CCOCH}_{3}\right)\) has a boiling point of \(56^{\circ} \mathrm{C}\). Based on the data given in Figure 11.25, would you expect acetone to have a higher or lower vapor pressure than ethanol at \(25^{\circ} \mathrm{C}\)?Text Transcription:(H_3CCOCH_3)56^{\circ} C25^{\circ} Cā€ is broken down into a number of easy to follow steps, and 38 words. Since the solution to 11.50 from 11 chapter was answered, more than 239 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Chemistry: The Central Science, edition: 14. The full step-by-step solution to problem: 11.50 from chapter: 11 was answered by , our top Chemistry solution expert on 10/03/18, 06:29PM. Chemistry: The Central Science was written by and is associated to the ISBN: 9780134414232.

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?Acetone \(\left(\mathrm{H}_{3} \mathrm{CCOCH}_{3}\right)\) has a boiling point of \(56^{\circ} \mathrm{C}\). Based on the data given in Figure 11.25,