Chemistry 102 Exam 3

• solvent - the one in larger amount, dissolving medium
• solute - the one in lesser supply, dissolves into solvent
• strong electrolytes - dissolves and dissociates readily, easily conducts electric current
• weak electrolytes - slow and low dissociation, only strong currents pass through
• non-electrolytes - no dissociation, no electricity passes through
• Molarity [M] = Mol of solute / Volume of solution (L)
• # mol of solute = volume of solution (L) * Molarity (M) in a dilution, # of moles of solute does not change -> C1V1 = C2V2
• Mass percentage = (mass of solute / total mass of solution) * 100
• Volume percentage = (volume of solute / volume of solution) * 100
• strong acid - dissolves readily in water to yield H3O+
• weak acid - dissolves less in water
• strong base - dissolves readily in water to yield OH-
• weak base - dissolves less in water
• neututralization - acid and base react to produce water and a salt
• oxidation - increasing of oxidation number of an element (loss of electrons)
• reduction - decreasing of oxidation number of an element (gain of electrons)
• oxidizing agent - reactant that causes oxidation
• reducing agent - reactant that causes reduction
• Amonton's/Gay-Lussac's Law: pressure is directly proportional to absolute temperature$P1/T1 =$$P2/T2$ **constants: n, V**
• Charle's Law: volume is directly proportional to absolute temperature **constants: n, P**$V1/T1 =$$V2/T2$
• Boyle's Law: volume is inversely proportional to pressure **constants: n, T**$P1V1 =$$P2V2$
• Avogrado's Law: volume is directly proportional to number of moles **constants: P, T**$V1/n1 =$$V2/n2$
• Ideal gas law: PV/nT = constant, PV=nRT
• Dalton's Law of Partial Pressures: for mixtures of gases in a container, total pressure exerted is the sum of partial pressure of each gas
• Kinetic Molecular Theory: 1. Gas molecules are in continuous random motion; traveling in straight lines until a collision happens, 2. gas molecules/atoms have negligible volume compared to the volume they occupy (V), 3. collisions between molecules/atoms and with the vessel wall exert pressure (P), 4. gas molecules/atoms exert no attractive forces on each other or on the vessel wall, 5. collisions are elastic, 6. Avereage Kinetic Energy of a gas is proportional to the absolute (kelvin) temperature of gas
• strong acids: HBr, HCl, HI, HNO3, HClO4, H2SO4
• strong bases: NaOH, KOH, Ba(OH)2, LiOH, RbOH, Sr(OH)2
• Kinetic energy of particle: $KE =$$1/2(mu^2)$
• $KE avg =$$3/2(RT)$ **only depends on temperature**
• Root mean square velocity/speed: $Urms =$$sqrt(3RT/M)$
• at same temperatures, gases will have the same KE avg but the gas with the smaller molar mass will have the higher speedee
• rate of effusion = amount of gas passing through an area / unit of time$effusion rate of gas A/effusion rate of gas B =$$sqrt(MB)/sqrt(MA)$
• higer molar mass -> slower rate of effusion
• Van der Waal's Equation: $(P + an^2/V^2)(V-nb) =$$nRT$
• real gas molecules have volume, so the actual volume available for a given gas molecule is less than V, the volume of the container **correction factor is subtracted**
• real gases have attractive intermolecular forces so the particles collide with the wall less and the real pressure is smaller **correction factor is added**
• real gases behave ideally at low pressures and high temperatures
• internal energy: $deltaE =$$q +$$w$
• endothermic: heat enters the system -> q is +
• exothermic: heat is given off by system -> q is -