CHM 101 1st Edition Lecture 13Lecture 12 Overview I. State FunctionsII. Types of WorkIII. EnthalpyLecture 13 OverviewI. Specific HeatII. CalorimetrySpecific heat – the amount of energy required to raise the temperature of an object by 1 degreeCelsius Specific heat capacity – the amount of energy required to raise the temperature of 1 gram of a substance by 1 degree CelsiusCs = q/m x ∆TCs – specific heatq – heatm – mass∆T – change in temperature - ∆T = Tfinal – Tinital Constants (which should be given to you in the problem, but it doesn’t hurt to be familiar with them)- N2 – 1.04- Al - 0.90These 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.- Fe – 0.45- Hg – 0.14- H2O – 4.18- CH4 – 2.20- CO2 – 0.84- CaCO3 – 0.82Example: It takes 16 J of thermal E (heat) to raise the temperature of 6.0 g of Al from 22 degreesCelsius to 25 degrees Celsius. What is the specific heat of Al?- Cs = (16 J)/ (6.0 g)(25 – 22)- Cs = 0.89 J/g CCalorimetry- The measurement of heat flow during physical and chemical changes - Calorimeter – device for measuring heat flow - Amount of heat lost from the system is equal to the heat absorbed by the surroundings qsystem = -qsurroundings- Final temperature of the system and surroundings will equal each otherDetermining Changes in Enthalpy using Calorimetry - The system in calorimetry may also be a chemical reaction (rxn). The solution is considered the surroundings.qsystem = qsurroundings qrxn = -Csoln x msoln x ∆Tsoln For quiz Friday- 5.1 – 5.2- Change in internal energy - Exothermic and Endothermic- Enthalpies of reactionso ∆Hrxn = Hproducts –
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