1 week of notes CHM 132
1 week of notes CHM 132 CHM 132
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This 2 page Class Notes was uploaded by Angel Carrasquillo on Sunday January 24, 2016. The Class Notes belongs to CHM 132 at University of Rochester taught by Dr. Hafensteiner in Spring 2016. Since its upload, it has received 54 views. For similar materials see CHM CONCEPTS, SYST, PRACT II in Chemistry at University of Rochester.
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Date Created: 01/24/16
Angel Carrasquillo Week of 01/17/1601/24/16 Chemistry 132 Notes ● Thermodynamics If q is positive, reaction is endothermic. If q is negative, reaction is exothermic. ● Constant Pressure ΔEsystem = qp + w = qp + (PΔv)(101.3J/L*atm) ΔE const. pressure = ΔEconst. volume At Const. Volume ΔE = qv ● Enthalpy heat that’s released under const. pressure situations. ΔG = ΔH TΔS ΔH = ΔE w → ΔH = qp + w w → ΔH = qp ● Calorimetry how energy flow is measured. (ΔH) open calorimeter, change in volume occurs (Δ V) closed calorimeter, no Δ V only qv ● Open calorimeter = constant pressure ● Specific Heat Capacity (Cs) = J/K*gram ● Molar Heat Capacity (Cn) = J/K*mol ● q solution = q reaction ● ΔH reaction = q solution reaction is endothermic, solution has increase in temperature ● q surroundings (solution) = nCnΔT or mCsΔT….n for mols, m for mass ● ΔV = Δ nRT/P ● When we have an expansion, work value is negative ● Molar heat capacity of an ideal gas KE = 3/2RT ΔKE = 3/2RΔT Cv = 3/2R Cp = 5/2R (Cn for volume and pressure for ideal gases) ● heating gas results in loss of energy as work ● ΔEv = ΔEp ΔE = nCvΔT = qv ΔE = nCpΔ T + w qp = nCpΔT = ΔH ● For real molecules, Cv > 3/2R, Cp > 5/2R ● Heats of Formation ΔHf Knot = standard conditions ( 25 celsius, 1 atm) making 1 mol of compound from elements ΔHf knot of elemental forms = 0