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Ch.11 - Liquids and Intermolecular Forces

Chapter 11, Problem 83a

(a) When you exercise vigorously, you sweat. How does this help your body cool?

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Hey, everyone were asked which of the following statement explains how sweat aids in cooling our bodies first. Let's think about what we know before we dive into our answer choices. So we know on the surface of our body we have evaporation of water, and we also know that the heat required for vaporization is absorbed from the body. So looking at our answer choices, we can already eliminate A and C. Since we're looking for water evaporates next, we know that if our body loses heat, then our body is subsequently cold. Now, looking back at our answer choices, it looks like d is going to be our answer since the body releases heat that is absorbed by the water on the surface and the water evaporates, which helps cool down our body. So I hope that made sense and let us know if you have any questions.
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The table below shows the normal boiling points of benzene and benzene derivatives.

(a) How many of these compounds exhibit dispersion interactions?

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The table below shows the normal boiling points of benzene and benzene derivatives. (e) Why is the boiling point of phenol the highest of all?

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Use the normal boiling points propane (C3H8) -42.1 °C butane (C4H10) -0.5 °C pentane (C5H12) 36.1 °C hexane (C6H14) 68.7 °C heptane (C7H16) 98.4 °C to estimate the normal boiling point of octane (C8H18). Explain the trend in the boiling points.

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Textbook Question

(b) A flask of water is connected to a vacuum pump. A few moments after the pump is turned on, the water begins to boil. After a few minutes, the water begins to freeze. Explain why these processes occur.

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Textbook Question

The following table gives the vapor pressure of hexafluorobenzene (C6F6) as a function of temperature: (a) By plotting these data in a suitable fashion, determine whether the Clausius–Clapeyron equation (Equation 11.1) is obeyed. If it is obeyed, use your plot to determine ∆Hvap for C6F6.

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Textbook Question

Suppose the vapor pressure of a substance is measured at two different temperatures. (a) By using the Clausius–Clapeyron equation (Equation 11.1) derive the following relationship between the vapor pressures, P1 and P2, and the absolute temperatures at which they were measured, T1 and T2: (b) Gasoline is a mixture of hydrocarbons, a component of which is octane (CH3CH2CH2CH2CH2CH2CH2CH3). Octane has a vapor pressure of 13.95 torr at 25 °C and a vapor pressure of 144.78 torr at 75 °C. Use these data and the equation in part (a) to calculate the heat of vaporization of octane. (c) By using the equation in part (a) and the data given in part (b), calculate the normal boiling point of octane. Compare your answer to the one you obtained from Exercise 11.81. (d) Calculate the vapor pressure of octane at - 30 °C.

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