Objectives Learning Chapter 10 Gases
CHEM 1411 (Brown, LeMay, and Bursten 10ed)
10.1 Characteristics of Gases
10.1a 10.2a Describe the characteristics of gases. (10.1) Explain atmospheric pressure and the use of the barometer; state the common units of pressure and convert between torr, mm Hg, and atmospheres. (10.2) Explain the relationship of the four variable, P, n, T, and V in Boyles Law, Charles Law, and Avogadros Law. (10.3) Perform calculations given the empirical gas laws: Boyle's Law, Charles' Law, Avogadros Law, the combined gas law, and the ideal gas law. (10.3-10.4) Determine gas densities or molar masses using the ideal gas law. (10.5) Work stoichiometry problems involving gases. (10.5-10.6) Perform calculations using Daltons law of partial pressures. (10.6) Describe the main points of the kinetic-molecular theory. (10.7) Perform calculations using rms speed and Grahams law of effusion. (10.8) Explain why real gases differ from ideal gases. (10.9)
10.2 Pressure
10.3 The Gas Laws
10.3a
10.4 The Ideal-Gas Equation
10.4a
10.5 Further Applications of the Ideal-Gas Equation
10.5a 10.5b 10.6a 10.7a 10.8a 10.9a
10.6 Gas Mixtures and Partial Pressures 10.7 Kinetic-Molecular Theory 10.8 Molecular Effusion and Diffusion 10.9 Real Gases: Deviations from Ideal Behavior
Learning Objectives Chapter 5 Thermochemistry
CHEM 1411 (Brown, LeMay, and Bursten 10ed)
5.1
5.1a 5.1b
The Nature of Energy
Explain the relationship between energy, work, and heat. (5.1) Convert between Joules and calories as units of energy. (5.1)
5.2
5.2a 5.2b
The First Law of Thermodynamics
State the first law of thermodynamics. State (5.2) the meaning of positive and negative values of E, q, and w. (5.2)
5.3
5.3a
Enthalpy
Explain the flow of heat from system to surroundings (or from surroundings to system) in a reaction in which the sign and magnitude of the change in enthalpy (H) are known. (5.2)
5.4
5.4a
Enthalpies of Reaction
Calculate moles, grams and/or heat absorbed from a balanced equation with a given Hrxn value. (5.4)
5.5
5.5a 5.5b 5.5c 5.5d
Calorimetry
Know the units for heat capacity, specific heat, and molar heat capacity. (5.5) Calculate the specific heat, the mass of substance, the heat absorbed, or the change in temperature for specific heat problems (q = s m T). (5.5) Explain the difference between the heats of reaction determined in Bomb Calorimetry and Coffee-cup Calorimetry (think constant volume vs. constant pressure). (5.5) Calculate the heat evolved in a reaction (or absorbed by the bomb calorimeter) using heat capacity and temperature change. (qrxn = -qcal = -Ccal T). (5.5)
5.6
5.6a
Hesss Law
Use Hesss law, the enthalpy guidelines, and the Hs of two or three known chemical equations to calculate H for a target chemical equation. (5.4 and 5.6)
5.7
5.7a 5.7b
Enthalpies of Formation
Analyze the chemical equation to determine if it represents a formation reactionthe reaction that the standard enthalpy of formation (Hf) describes. (5.7) Use Hf to calculate standard enthalpies of reaction (H). (5.7)
5.8
5.8a
Food and Fuels
Recognize different sources of energy that we use and environmental issues related to them: food, solar, fossil fuels, wind, nuclear, geothermal, hydroelectric, and biomass. (5.8)