The Ideal Gas Law Quiz

PDF page 596: where is the absolute pressure of a gas, is the volume it occupies, is the number of atoms and molecules

PDF page 596: in the gas, and is its absolute temperature. The constant is called the Boltzmann constant in honor of Austrian physicist Ludwig Boltzmann (1844–1906) and has the value 13.19

PDF page 596: The ideal gas law can be derived from basic principles, but was originally deduced from experimental measurements of Charles’ law (that volume occupied by a gas is proportional to temperature at a fixed pressure) and from Boyle’s law (that for a fixed temperature, the product is a constant). In the ideal gas model, the volume occupied by its atoms and molecules is a negligible fraction of . The ideal gas law describes the behavior of real gases under most conditions. (Note, for example, that is the total number of atoms and molecules, independent of the type of gas.) Let us see how the ideal gas law is consistent with the behavior of filling the tire when it is pumped slowly and the temperature is constant. At first, the pressure is essentially equal to atmospheric pressure, and the volume increases in direct proportion to the number of atoms and molecules put into the tire. Once the volume of the tire is constant, the equation predicts that the pressure should increase in proportion to the number N of

PDF page 596: The ideal gas law can be derived from basic principles, but was originally deduced from experimental measurements of Charles’ law (that volume occupied by a gas is proportional to temperature at a fixed pressure) and from Boyle’s law (that for a fixed temperature, the product is a constant). In the ideal gas model, the volume occupied by its atoms and molecules is a negligible fraction of . The ideal gas law describes the behavior of real gases under most conditions. (Note, for example, that is the total number of atoms and molecules, independent of the type of gas.) Let us see how the ideal gas law is consistent with the behavior of filling the tire when it is pumped slowly and the temperature is constant. At first, the pressure is essentially equal to atmospheric pressure, and the volume increases in direct proportion to the number of atoms and molecules put into the tire. Once the volume of the tire is constant, the equation predicts that the pressure should increase in proportion to the number N of

PDF page 596: The ideal gas law can be derived from basic principles, but was originally deduced from experimental measurements of Charles’ law (that volume occupied by a gas is proportional to temperature at a fixed pressure) and from Boyle’s law (that for a fixed temperature, the product is a constant). In the ideal gas model, the volume occupied by its atoms and molecules is a negligible fraction of . The ideal gas law describes the behavior of real gases under most conditions. (Note, for example, that is the total number of atoms and molecules, independent of the type of gas.) Let us see how the ideal gas law is consistent with the behavior of filling the tire when it is pumped slowly and the temperature is constant. At first, the pressure is essentially equal to atmospheric pressure, and the volume increases in direct proportion to the number of atoms and molecules put into the tire. Once the volume of the tire is constant, the equation predicts that the pressure should increase in proportion to the number N of

PDF page 595: Figure 13.17. Because atoms and molecules have large separations, forces between them can be ignored, except

PDF page 596: FIGURE 13.17 Atoms and molecules in a gas are typically widely separated, as shown. Because the forces between them are quite weak at

PDF page 595: of two or more atoms. We will primarily use the term “molecule” in discussing a gas because the term can also be applied to monatomic gases, such as helium.) Gases are easily compressed. We can see evidence of this in Table 13.2, where you will note that gases have the largest coefficients of volume expansion. The large coefficients mean that gases expand and contract very rapidly with temperature changes. In addition, you will note that most gases expand at the same rate, or have the same . This raises the question as to why gases should all act in nearly the same way, when liquids and solids have widely varying expansion rates. The answer lies in the large separation of atoms and molecules in gases, compared to their sizes, as illustrated in

PDF page 595: of two or more atoms. We will primarily use the term “molecule” in discussing a gas because the term can also be applied to monatomic gases, such as helium.) Gases are easily compressed. We can see evidence of this in Table 13.2, where you will note that gases have the largest coefficients of volume expansion. The large coefficients mean that gases expand and contract very rapidly with temperature changes. In addition, you will note that most gases expand at the same rate, or have the same . This raises the question as to why gases should all act in nearly the same way, when liquids and solids have widely varying expansion rates. The answer lies in the large separation of atoms and molecules in gases, compared to their sizes, as illustrated in

PDF page 598: It is sometimes convenient to work with a unit other than molecules when measuring the amount of substance. A mole (abbreviated mol) is defined to be the amount of a substance that contains as many atoms or molecules as there are atoms in exactly 12 grams (0.012 kg) of carbon-12. The actual number of atoms or molecules in one mole is called Avogadro’s number , in recognition of Italian scientist Amedeo Avogadro (1776–1856). He developed the concept of the mole, based on the hypothesis that equal volumes of gas, at the same pressure and temperature, contain equal numbers of molecules. That is, the number is independent of the type of gas. This hypothesis has been confirmed, and the value of Avogadro’s number is 13.28

PDF page 598: It is sometimes convenient to work with a unit other than molecules when measuring the amount of substance. A mole (abbreviated mol) is defined to be the amount of a substance that contains as many atoms or molecules as there are atoms in exactly 12 grams (0.012 kg) of carbon-12. The actual number of atoms or molecules in one mole is called Avogadro’s number , in recognition of Italian scientist Amedeo Avogadro (1776–1856). He developed the concept of the mole, based on the hypothesis that equal volumes of gas, at the same pressure and temperature, contain equal numbers of molecules. That is, the number is independent of the type of gas. This hypothesis has been confirmed, and the value of Avogadro’s number is 13.28

PDF page 598: One mole always contains particles (atoms or molecules), independent of the element or substance. A mole of any substance has a mass in grams equal to its molecular mass, which can be calculated

PDF page 598: One mole always contains particles (atoms or molecules), independent of the element or substance. A mole of any substance has a mass in grams equal to its molecular mass, which can be calculated