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