CHEM 1110 1st Edition Lecture 12Outline of Last Lecture I. The 1st law of Thermodynamics II. Enthalpy III. Enthalpies of reactionOutline of Current Lecture I. Enthalpies of reaction II. Calorimetry Current LectureI. Enthalpies of reaction A. Thermochemical equations: Summery of the relationship between amount (mol) of substance and the heat (kJ) transferred during a reaction 1. A -> B +/- HEATII. CalorimetryA. Caloimetry- measurement of heat flow B. Heat capacity (C)- is the amount of heat required to raise the temperature of an object by 1 K or (1 degree C) (extensive)1. C= q/∆T [q:J; ∆T:K]2. Water= 4.184 (J/gK)C. Specific heat capacity (Cs)- the amount of heat required to raise 1 g by 1 K (intensive)1. (Cs)+q/(mass x ∆T) [q:J; T:K; c: J/(gK)]D. Heat change: q= mC∆TThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.E. Molar Heat Capacity (Cm): the amount required to raise one mole by 1 K (intensive)F. Constant- Pressure Calorimetry1. Used to measure heat changes in noncombustion reactions 2. 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 G. System and Surroundings 1. System- the chemical reaction 2. Surroundings- the solution and the calorimeter 3. Energy is Conserved- Heat lost = heat gained a. qsolution+ qcalorimeter+
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