MCAT Gen Chem 2
Card Set Information
MCAT Gen Chem 2
Whether or not a process or reaction can occur.
How fast or slow a process or rection can occur.
Exothermic energy coordinate diagram
Endothermic energy coordinate diagram
Fluid movement caused by the hotter portions of a fluid rising and the cooler portions of a fluid sinking.
Electromagnetic waves emitted from a hot body into the surrounding environment.
Light colors radiate and absorb less
Dark colors radiate and absorb more
Black Body Radiator - perfect theoretical radiator
Molecular collisions along a conduit
Analogous to current flow through a wire or H
O through a pipe
Heat Capacity (definition)
The amount of energy (in Joules or Calories) a system can absorb per temperature unit (J/K or cal/˚C).
Heat Capacity (formula)
C = q/∆T
Specific Heat Capacity (definition)
Is for a given substance only and is defined as the heat capacity per unit mass.
Specific Heat Capacity (formula)
q = mc∆T
Specific Heat of Water
First Law of Thermodynamics
∆E = q + w
Work done on the system (+)
Work done by the system (–)
Second Law of Thermodynamics
Heat cannot be changed completely into work in a cyclical process
Entropy in an isolated system can never decrease
Third Law of Thermodynamics
Pure substances at absolute zero have an entropy of zero
Zeroth Law of Thermodynamics
Celsius – Kelvin conversion
0˚ C = 273.15 K
-273.15˚ C = 0 K
Absolute zero = 0 K
Kinetic Energy of Gasses (formula)
KE = 3/2kT
k = Boltzman's constant (1.3806503 e
m2 kg s-2 K-1)
The energy contained within chemical bonds or HEAT
A measure of the randomness or disorder in a system
Standard State is 25˚ C (298K) and ∆H = 0
*For thermodynamics problems
STP (standard temperature and pressure) is 0˚ Celsius (273K) and 1 atm
*For gas problems
+ ∆S =
Increased randomness, energy released and available to do work
– ∆S =
Decreased randomness, energy is required to "create" increased order and that energy is thus unavailable to do work
Entropy (∆S) increases with: (5 things)
1. Increased number of items/particles/etc.
(Gas trumps # of moles or particles. This means that if two moles of reactants makes one mole of product and that product is a gas, it is still +∆S)
2. Increased volume
3. Increased temperature
4. Increased disorder
5. Decreased pressure (the higher the pressure the more packing and order of molecules)
Gibbs Free Energy (∆G)
∆G = the amount of "free" or "useful" energy available to do work.
-∆G = Spontaneous; exothermic
+∆G = Non-spontaneous; endothermic
Rate Order Graphs
: [A] vs. time is linear with slope -k
: ln[A] vs. time is linear with slope -k
: 1/[A] vs. time is linear with slope k
: 1/2[A]2 vs. time is linear with slope k
Fundamental Thermodynamic Relation formula
∆G = ∆H - T∆S
∆G - Gibbs
∆H - Enthalpy
∆S - Entropy
T - Temp K
(+) means more disorder or increased entropy.
(–) means more order or decreased entropy.