week 7 energy Flashcards
Energy
The capacity to do work
Work
measurement of the total internal energy
law of conservation of energy
Can’t be created or destroyed only transformed
2 law of Thermodynamics
Natural Processes lead to spatial homogeneity of matter and energy
What happens to entropy when temperature approaches 0
Entropy approaches a constant value
Types of Energy
Potential Kinetic
Units of Energy
J Joule
1J is the amount of energy required to apply 1N of force over a distance of 1M
Entropy
Disorder in the system
- universe wants disorder-
Enthalpy
Measure of total
Exothermic
Energy is transferred from the system into the surroundings
Delta H negative (System net loss of energy)
Endothermic
Energy transferred from surroundings into the system
Delta H positive (System net gain of energy)
Exergonic
Energetic and spontanrous
Endergonic
Requires energy and not spontaneous
Delta H
Change in enthalpy (a measure of total energy)
Activation energy
Energy peak/barrier required for the reaction to occur
Gibbs Free Energy
Energy Present in a System
- an indicator of spontaneity
Delta G = Delta H (Enthalpy) - T (temp) . Delta S (Entropy)
Delta G must be negative to be spontaneous
Delta S positive
Delta H negative
Delta S
Change in Entropy ( difference between order and chaos, how spontaneous a reaction is)
How to make a reaction more spontaneous
Enzymes lower activation energy to create scenarios where the reaction is favourable
λ (lambda)
Wavelength
Beer-Lambert Equation
A=E l C
A - Absorbance
E - Molar extinction coefficient (mol^-1cm^-1
l - Path Lentgh (cm)
C - Concentration (M) or (mol/L)
