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MCAT Chemistry
MCAT Chemistry
19
Chemistry
Undergraduate 3
01/01/2009

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Cards

Term
Factors that affect the rate of reaction
Definition
Catalysts, Medium, Temperature, Concentration of Reactants
Term
Homogeneous catalysts
Definition
Catalysts are in the same phase as the reactant
Term
Heterogeneous Catalysts
Definition
Catalysts are in a different phase from the reactants
Term
Enthalpy
Definition
is the heat absorbed or evolved by a system at constant pressure
Term
kinetic molecular theory
Definition
no volume, no attractions or repulsions, ave KE is proportional to abs temp, elastic collisions, continuous random motion
Term
KE formula
Definition
1/2 mv^2 = 3/2kT
Term
Diffusion
Definition
The flow of gas particles through a mixture e.g. the smell from an open bottle of perfume diffusing across the room. Isobaric and Isothermal. r1/r2 = (mr2/mr1)^1/2
Term
Effusion
Definition
the flow of gas particles under pressure from one compartment to another through a small opening. isothermal. r1/r2 = (mr2/mr1)^1/2
Term
Boyle's Law
Definition
P1V1=P2V2
Term
Charles's Law
Definition
V1/T1 = V2/T2
Term
Avogadro's Principle
Definition
n1/V1 = n2/V2
Term
Ideal Gas Equation and Encompassing Gas Eqtn
Definition
PV = nRT
P1V1/T1 = P2V2/T2
Term
Density
Definition
m/V
Term
STP
Definition
273.15K. 1 atm amd 22.4L/mol
Kinetics
Term
Standard Conditions
State functions
Definition
293.15K and 1 atm
Enthalpy, Entropy, Gibb's free energy
Term
Ideal gas behaviour - exception
Definition
seen at low pressure and high temperature. Exception = high pressure and low temperature bc molecular volume and intermolecular attraction become important
Term
Dalton's Law of Partial Pressure
Definition
Pa = XaPt where X = mole fraction & Pt = total pressure
Term
Mole Fraction
Definition
Xa = na (moles of A) /nt (total moles)
Term
Root mean square
Definition
is the speed which corresponds to the ave. KE per particle. Urms = (3RT/mr)^1/2
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