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CHEM 1120: cp12cp13
henrys law |
C=k*P
C=concentration in M(molarity)
k=constant (mol/L*atm)
p=pressure atm |
Molarity |
Molarity = (moles of solute)/(liters of solution) |
molality (m) |
mole of solute/mass of solvent (kg) |
freezing point depression |
delta Tf=-Kf*m
Kf=constant C/m
m=molality |
boiling point elevation |
delta Tb=Kb*m
Kb=constant C/m
m=molality |
Osmotic Pressure |
pi = (MRT)i
M=molarity
R=ideal gas
T=kelvin
i=electoryle intergaer |
solubility of gas |
solubility=k*P
k=constant (mol/L*atm)
P=partial pressure of gas over solution |
what affects rate of reaction |
temperature
pressure
surface area
catalyst
concentration |
Order of Reactions |
zero order=K
first order=k*[A]
second order=k*[A]^2 |
Half-life |
The time it takes for half the sample to decay. |
Identify Zero Order |
When [A or B] is changed, but rate remains the same. This is zero order |
identify first order reaction |
When x[A or B] is the same as the rate increase. IE 3[A] 3=3^1 |
identify second order reaction |
Dependent on concentration of two reactants m+n+..=2 IE
2[A] makes ratex4 is 4=2^2
3[A] rate x9
|
how to find k constant |
k=(rate/(A^m*B^n)) |
Solve for initial rate |
initial rate=k*A^m*B^n |
3 factors in chemical kinetics |
collision frequency-rate of collisions
Activation Energy-min energy above avg kinetic needed to trigger reaction
orientation-molecules require proper alignment |
Effect of temperature on reaction rates |
rate constant K changes with temperature, activation energy is the same, higher temp allows more molecules to have enough energy to overcome the activation energy barrier |
Arrhenius Equation |
k(T)=Ae^(-Ea/RT), A=Ahrrenius factor, R=8.314, T=temperature, Ea= activation energy |
two types of catalysts |
homogenous-catalyst exists same phase as reactants
heterogenous-catalysts exists in a different phase than reactants |