CHEM 111 1st EditionExam # 2 Study Guide Lectures: 12-19Chapter 5: Thermochemistry (February 16- 23)Explain energy and work.Energy is the capacity to do work or transfer or transfer heat. Work is energy transferred when an object is moved by a force What is the formula for work?W= F x d [F=force, d= distance] [F= mass x acceleration (9.8)]What is heat (or thermal energy)?Energy transferred between objects as a result of different temperatures.What is Thermodynamics?The study of energy and its transformations.What is Thermochemistry?The study of chemical reactions and energy changes involving heatWhat are the 2 fundamental forms of energy? Explain them.Kinetic energy which is due to the motion of an object E = 1/2mv2 = J and potential energy which is due to the position or condition of an objectWhat is the 1st Law of Thermodynamics?Total energy of the universe is constant; if the system loses energy, it must be gained by the surroundings and vice versa; Transfer of internal Energy (E) between a system and its surroundings.What is a State Function?A property of a system that depends only on its current state and not on the manner in which the state was achieved Are heat and work a state function?No.What are considered state functions?Temperature, volume, pressure, and internal energy.What is Enthalpy?Heat in processes occurring at constant pressure when the only work is PV work.What is Calorimetry?The measurement of heat flow.What is heat capacity?The amount of heat required to raise the temperature of an object by 1 K or (1 degree C) (extensive)What is constant- Pressure Calorimetry?It is used to measure heat changes in non-combustion reactions; by carrying out a reaction in aqueous solution in a simple calorimeter such as this one, one can indirectly measure the heat change for the system by measuring the heat change for the water in the calorimeter.Explain Hess’s Law.If a reaction is carried out in a series of steps, delta H for the overall reaction equals the sum of the enthalpy changes for the individual steps.Chapter 10: Gases (February 25-March 2)Explain the characteristics of gases.A gas is a physical state of an element or compound. Gases expand to fill the entire container they are placed in. They move rapidly around container & exert force on its walls. Gases have low densities, thus they are easily compressed into smaller volumes. Gases (ideally) interact weakly with other gases and often are highly miscible.What are the Elemental gases?He, Ne, Ar, Kr, Xe, and H2, O2, N2, F2, Cl2True or False: The density of a gas is directly proportional to its molar mass.True.Explain Dalton’s law of Partial pressures.The total pressure of a mixture of gases equals the sum of the partial pressures that each gas would exert if it were alone (in the same container)What is Kinetic Molecular theory? A theory that describes microscopic (molecular) properties and explains gas behavior in terms of the gas particle motion (atoms or molecules).What are some assumptions about the K-M Theory?The gas particles in an ideal system: are present in large numbers with continuous , random motion, have negligible volumes compared to its container volume, exert no attractive or repulsive forces on each other so intermolecular forces are negligible, collide with each otherand the walls of their container, but (at constant T) their average kinetic energy is unchanged.What is the difference between diffusion and effusion?Diffusion is the net path of gas while Effusion is through pinhole.Explain Graham’s law of Effusion.The effusion rate of gas is inversely proportional to the square root of its molar mass. Only those molecules that hit the small hole will escape through it. Therefore, the high the U the greater the probability of a gas molecule hitting the hole.Chapter 15: Chemical Equilibrium (March 2-6)Explain chemical equilibrium.A reaction is reversible and is in a state of constant exchange (equilibrium is dynamic) where the forward rate of reaction is matched by the reverse reaction. Reactant/product concentrations do not change with time for a given reaction (after it reaches equilibrium.Explain the Haber process.At equilibrium, the concentration of reactants and products no longer change. For equilibrium to occur, neither reactants nor products can escape from the system. At equilibrium, a particular ratio of concentration terms equal a constant.What if K is much greater than 1?The reaction is product-favored; product predominates at equilibrium.What if K is much less than 1?The reaction is reactant-favored; reactant predominates at