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Chapter 6: Problem 131

Briefly describe each concept or process: (a) absolute zero of temperature; (b) collection of a gas over water; (c) effusion of a gas; (d) law of combining volumes.

Short Answer

Expert verified
Absolute Zero is the minimum theoretical temperature, set as 0 Kelvin or -273.15 Celsius. Collection of a gas over water is a laboratory method to measure gas produced in a chemical reaction. Effusion of a gas is when it escapes from a container through a tiny hole into an evacuated space, explained by Graham's law. The law of combining volumes, or Gay-Lussac's law, states that the volume ratios of gases in a reaction are proportional to the stoichiometric ratios.

Step by step solution

01

Define Absolute Zero

Absolute zero is the lowest possible temperature where nothing could be colder and no heat energy remains in a substance. It is precisely set as 0 Kelvin, or -273.15 degrees Celsius.
02

Describe the Collection of a Gas Over Water

The Collection of a gas over water is a common laboratory method used to collect the gas produced from a chemical reaction. It is done by displacing water in a container with the gas, which can then be measured. However, the collected gas is often saturated with water vapor, which must be taken into account during calculations.
03

Define Effusion of a Gas

Effusion is a process in which a gas escapes from a container through a tiny hole into an evacuated space. It is described quantitatively by Graham's law, which states that the rate of effusion of a gas is inversely proportional to the square root of its molecular weight.
04

Explain the Law of Combining Volumes

The law of combining volumes, also known as Gay-Lussac's law, states that the ratio of the volumes of gases involved in a chemical reaction will be directly proportional to the ratio of stoichiometric coefficients in the balanced chemical equation, provided all gases are at the same temperature and pressure.

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Most popular questions from this chapter

What is the volume, in liters, occupied by a mixture of 15.2 \(\mathrm{g} \mathrm{Ne}(\mathrm{g})\) and \(34.8 \mathrm{g} \mathrm{Ar}(\mathrm{g})\) at 7.15 atm pressure and \(26.7^{\circ} \mathrm{C} ?\)

A sample of \(\mathrm{O}_{2}(\mathrm{g})\) is collected over water at \(24^{\circ} \mathrm{C}\) The volume of gas is 1.16 L. In a subsequent experiment, it is determined that the mass of \(\mathrm{O}_{2}\) present is 1.46 g. What must have been the barometric pressure at the time the gas was collected? (Vapor pressure of water \(=22.4 \text { Torr. })\)

Determine \(u_{\mathrm{m}}, \bar{u},\) and \(u_{\mathrm{rms}}\) for a group of ten automobiles clocked by radar at speeds of 38,44,45,48,50 \(55,55,57,58,\) and \(60 \mathrm{mi} / \mathrm{h},\) respectively.

Appendix E describes a useful study aid known as concept mapping. Using the method presented in Appendix \(\mathrm{E}\), construct a concept map illustrating the different concepts to show the relationships among all the gas laws described in this chapter.

A \(0.156 \mathrm{g}\) sample of a magnesium-aluminum alloy dissolves completely in an excess of \(\mathrm{HCl}(\mathrm{aq}) .\) The liberated \(\mathrm{H}_{2}(\mathrm{g})\) is collected over water at \(5^{\circ} \mathrm{C}\) when the barometric pressure is 752 Torr. After the gas is collected, the water and gas gradually warm to the prevailing room temperature of \(23^{\circ} \mathrm{C} .\) The pressure of the collected gas is again equalized against the barometric pressure of 752 Torr, and its volume is found to be \(202 \mathrm{mL}\). What is the percent composition of the magnesium-aluminum alloy? (Vapor pressure of water: \(6.54 \mathrm{mmHg}\) at \(5^{\circ} \mathrm{C}\) and \(21.07 \mathrm{mmHg}\) at \(\left.23^{\circ} \mathrm{C}\right)\)
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