In this lesson our instructor talks about calorimetry. He discusses heat capacity, molar heat capacity, constant pressure calorimetry, and constant volume calorimetry. In addition, he does three complete example problems.
Specific Heat: Amount of heat(Energy) required to raise the temp of 1 g of a substance by 1°C. Unit is J/g°C.
Heat lost/gained by a substance in a process is q=mCΔT m is mass in grams C is Heat Capacity of the substance ΔT is the Temperature Change experienced by the substance.
Constant Pressure Calorimetry: Heat lost/gained by one substance equals heat gained/lost by other substance. One of the substances is usually water: q1 = −q2
Constant Volume Calorimetry: Mass and Heat Capacity are combined into a single Heat Capacity for the apparatus, Cm, so the equation becomes: q = CmΔT
Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.