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e The one formula is double the formula of the other Thus, the smaller molecule dimerizes to produce the larger molecule You get 1 point if you combined two of the smaller molecules Total your points There are 9 points possible
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The mole is the amount of substance that contains the same number of particles as exactly 12 g of carbon-12 Avogadro s number is the number of particles per mole, 6022 1023 particles A mole is also the formula (atomic, molecular) mass expressed in grams If you have any one of the three moles, grams, or particles you can calculate the others The empirical formula indicates which elements are present and the lowest whole-number ratio The molecular formula tells which elements are present and the actual number of each Be able to calculate the empirical formula from percent composition data or quantities from chemical analysis Stoichiometry is the calculation of the amount of one substance in a chemical equation by using another one Always use the balanced chemical equation in reaction stoichiometry problems Be able to convert from moles of one substance to moles of another, using the stoichiometric ratio derived from the balanced chemical equation In working problems that involve a quantity other than moles, sooner or later it will be necessary to convert to moles The limiting reactant is the reactant that is used up first Be able to calculate the limiting reactant by the use of the mol/coefficient ratio Percent yield is the actual yield (how much was actually formed in the reaction) divided by the theoretical yield (the maximum possible amount of product formed) times 100% A solution is a homogeneous mixture composed of a solute (species present in smaller amount) and a solvent (species present in larger amount) Molarity is the number of moles of solute per liter of solution Be able to work reaction stoichiometry problems using molarity Always use the balanced chemical equation in reaction stoichiometry problems
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CHAPTER
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IN THIS CHAPTER Summary: Of the three states of matter gases, liquids, and solids gases are probably the best understood and have the best descriptive model While studying gases in this chapter you will consider four main physical properties volume, pressure, temperature, and amount and their interrelationships These relationships, commonly called gas laws, show up quite often on the AP exam, so you will spend quite a bit of time working problems in this chapter But before we start looking at the gas laws, let s look at the Kinetic Molecular Theory of Gases, the extremely useful model that scientists use to represent the gaseous state
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Gas constant, R = 00821 L atm mol 1 K 1
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r1 M2 = r2 M1
urms = root-mean-square speed r = rate of effusion STP = 0000 C and 1000 atm PV = nRT n 2a P + 2 (V nb ) = nRT V
PA = Ptotal XA, where XA = Ptotal = PA + PB + PC +
moles A totalmoles
102 U
Gases 103
PV1 P2V2 1 = T1 T2
urms =
3kT 3RT = m M
KE per molecule = 1/2 mv2 KE per mole = 3 RT 2
1 atm = 760 mm Hg = 760 torr
Kinetic Molecular Theory
KEY IDEA
The Kinetic Molecular Theory attempts to represent the properties of gases by modeling the gas particles themselves at the microscopic level There are five main postulates of the Kinetic Molecular Theory: 1 Gases are composed of very small particles, either molecules or atoms 2 The gas particles are tiny in comparison to the distances between them, so we assume that the volume of the gas particles themselves is negligible 3 These gas particles are in constant motion, moving in straight lines in a random fashion and colliding with each other and the inside walls of the container The collisions with the inside container walls comprise the pressure of the gas 4 The gas particles are assumed to neither attract nor repel each other They may collide with each other, but if they do, the collisions are assumed to be elastic No kinetic energy is lost, only transferred from one gas molecule to another 5 The average kinetic energy of the gas is proportional to the Kelvin temperature A gas that obeys these five postulates is an ideal gas However, just as there are no ideal students, there are no ideal gases: only gases that approach ideal behavior We know that real gas particles do occupy a certain finite volume, and we know that there are interactions between real gas particles These factors cause real gases to deviate a little from the ideal behavior of the Kinetic Molecular Theory But a non-polar gas at a low pressure and high temperature would come pretty close to ideal behavior Later in this chapter, we ll show how to modify our equations to account for non-ideal behavior Before we leave the Kinetic Molecular Theory (KMT) and start examining the gas law relationships, let s quantify a couple of the postulates of the KMT Postulate 3 qualitatively describes the motion of the gas particles The average velocity of the gas particles is called the root mean square speed and is given the symbol urms This is a special type of average speed
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