In this lecture you will learn about Energy in Chemical Reactions. Professor Goldwhite will first start with the two Forms of Energy, Potential Energy and Kinetic Energy. Next you will cover Units of Energy such as the Calorie before moving into Conservation of Energy with the First Law of Thermodynamics. Heat Capacity and Measurement is next on the agenda with the Calorimeter before you cover Enthalpy and its changes. You will learn about Exothermic Processes and Endothermic Processes with examples before covering Reversing a Process. Lastly are Hess's Law and the Enthalpy of Formation before you finish off with more examples.
forms of energy are kinetic from motion and potential
from position or chemical composition
units of energy: SI Joule; the Calorie in nutrition; Cal =
1000cal = 4.18kJ
is conserved in changes: not created or destroyed First Law of
definition of heat capacity, and how to measure it.
is heat energy change at constant pressure
calorimeter useful for determining enthalpy changes of chemical and
physical changes, including changes of phase
means heat energy leaves the system to surroundings (feels hot)
means heat energy enters the system from surroundings (feels cold)
Law a First Law statement treat enthalpy changes by algebra
definition of Standard Enthalpy of Formation, DH0
examples on using Standard Enthalpies of Formation to calculate
enthalpy changes in reactions etc.
Energy in Chemical Reactions
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.
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