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Chapter 5: Problem 27

List the characteristics of an ideal gas. Write the ideal gas equation and also state it in words. Give the units for each term in the equation.

Short Answer

Expert verified
The ideal gas law, \(PV = nRT\), describes the behavior of an ideal gas. It states that the product of the pressure and volume of a gas equals the product of the number of moles of the gas, the gas constant, and the absolute temperature. In this equation, pressure is measured in pascals, volume in cubic meters, the number of moles in moles, the gas constant in J/(mol.K), and temperature in Kelvin.

Step by step solution

01

Listing the Characteristics of an Ideal Gas

An ideal gas has the following characteristics: \n1. It consists of a large number of identical molecules.\n2. The intermolecular distance is far greater than the size of the molecules.\n3. The molecules are in constant random motion.\n4. Collisions between the molecules are perfectly elastic.\n5. There are no forces of attraction between the molecules.
02

Writing the Ideal Gas Law

The ideal gas law is given by the equation \(PV = nRT\), where:\n'P' is the pressure\n'V' is the volume\n'n' is the number of moles of the gas\n'R' is the universal gas constant\n'T' is the absolute temperature (measured in Kelvin)
03

Stating the Ideal Gas Law in Words

In words, the ideal gas law states that the product of the pressure and the volume of a gas is equal to the product of the number of moles of the gas, the universal gas constant, and the absolute temperature.
04

Stating the Units of Terms in the Ideal Gas Law

In the ideal gas equation, the units are as follows:\n'P' (pressure) is measured in pascal (Pa).\n'V' (volume) is measured in cubic meters (m^3).\n'n' (number of moles) is measured in moles (mol).\n'R' (universal gas constant) has a value of 8.314 J/(mol.K)\n'T' (temperature) is measured in Kelvin (K).

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Most popular questions from this chapter

Acidic oxides such as carbon dioxide react with basic oxides like calcium oxide (CaO) and barium oxide \((\mathrm{BaO})\) to form salts (metal carbonates). (a) Write equations representing these two reactions. (b) A student placed a mixture of \(\mathrm{BaO}\) and \(\mathrm{CaO}\) of combined mass \(4.88 \mathrm{~g}\) in a 1.46 - \(\mathrm{L}\) flask containing carbon dioxide gas at \(35^{\circ} \mathrm{C}\) and \(746 \mathrm{mmHg}\). After the reactions were complete, she found that the \(\mathrm{CO}_{2}\) pressure had dropped to \(252 \mathrm{mmHg}\). Calculate the percent composition by mass of the mixture. Assume volumes of the solids are negligible.

A sample of nitrogen gas kept in a container of volume \(2.3 \mathrm{~L}\) and at a temperature of \(32^{\circ} \mathrm{C}\) exerts a pressure of 4.7 atm. Calculate the number of moles of gas present.

A student breaks a thermometer and spills most of the mercury (Hg) onto the floor of a laboratory that measures \(15.2 \mathrm{~m}\) long, \(6.6 \mathrm{~m}\) wide, and \(2.4 \mathrm{~m}\) high. (a) Calculate the mass of mercury vapor (in grams) in the room at \(20^{\circ} \mathrm{C}\). The vapor pressure of mercury at \(20^{\circ} \mathrm{C}\) is \(1.7 \times 10^{-6} \mathrm{~atm} .\) (b) Does the concentration of mercury vapor exceed the air quality regulation of \(0.050 \mathrm{mg} \mathrm{Hg} / \mathrm{m}^{3}\) of air? (c) One way to treat small quantities of spilled mercury is to spray sulfur powder over the metal. Suggest a physical and a chemical reason for this action.

Compare the root-mean-square speeds of \(\mathrm{O}_{2}\) and \(\mathrm{UF}_{6}\) at \(65^{\circ} \mathrm{C}\)

Under the same conditions of temperature and pressure, which of the following gases would behave most ideally: Ne, \(\mathrm{N}_{2}\), or \(\mathrm{CH}_{4}\) ? Explain.
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