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Chapter 1: Q. 1.19 (page 13)
Suppose you have a gas containing hydrogen molecules and oxygen molecules, in thermal equilibrium. Which molecules are moving faster, on average? By what factor?
Hydrogen molecule will be moving faster
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List all the degrees of freedom, or as many as you can, for a molecule of water vapor. (Think carefully about the various ways in which the molecule can vibrate.)
Put a few spoonfuls of water into a bottle with a tight lid. Make sure everything is at room temperature, measuring the temperature of the water with a thermometer to make sure. Now close the bottle and shake it as hard as you can for several minutes. When you're exhausted and ready to drop, shake it for several minutes more. Then measure the temperature again. Make a rough calculation of the expected temperature change, and compare.
Consider the combustion of one mole of methane gas:
The system is at standard temperature and pressure both before and after the reaction.
(a) First imagine the process of converting a mole of methane into its elemental constituents (graphite and hydrogen gas). Use the data at the back of this book to find for this process.
(b) Now imagine forming a mole of and two moles of water vapor from their elemental constituents. Determine for this process.
(c) What is for the actual reaction in which methane and oxygen form carbon dioxide and water vapor directly? Explain.
(d) How much heat is given off during this reaction, assuming that no "other" forms of work are done?
(e) What is the change in the system's energy during this reaction? How would your answer differ if theended up as liquid water instead of vapor?
(f) The sun has a mass ofand gives off energy at a rate of watts. If the source of the sun's energy were ordinary combustion of a chemical fuel such as methane, about how long could it last?
Make a rough estimate of thermal conductivity of helium at room temperature. Discuss your result, explaining why it differs the value for air
Derive the equation 1.40 from the equation 1.39
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