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Rate at which two gases diffuse
r= rate
m= molar masses of each gas
Boyle's law - relating volume and pressure
PV = k
or
P
1
V
1
= P
2
V
2
moles and temperature are constant (isothermal)
Charle's law - relating volume and temperature
or
Dalton's law of partial pressures
Pressure of a gas
X = mols of species/total moles
Gram equivalent weight
n = number of monovalent particles produced
Number of equivalents
Rate law
Equilibrium constant
reaction quotient
Q
c
same as equilibrium constant
Enthalpy
positive change in enthalpy - endothermic
negative change in enthalpy - exothermic
Standard heat of a reaction - ΔH
o
rxn
ΔH
o
rxn
=
Same reaction for standard enthalpy and gibbs free energy of a reaction
Enthalpy of a reaction
ΔH(reactants to products) + ΔH(products to reactants
for all state functions
Entropy
Gibbs Free energy
positive change in free energy - nonspontaneous
negative change in free energy - spontaneous
Change in free energy with respect to k
eq
higher equilibrium constant = more negative change in free energy = more spontaneous
Determining free energy for a rxn in progress
Author
misbah
ID
220876
Card Set
Chemistry
Description
..
Updated
5/24/2013, 12:19:30 AM
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