## MCAT General Chemistry Review 2

 STP
 0oC and 1 atm
 Kinetic Molecular Theory
 Model of an ideal gas: -No volume -No forces (but repulsive due to collisions) -Completely elastic collision -Kinetic Energy is directly proportional to temperature
 Ideal Gas Law
 PV=nRT (R=0.08206 L atm K-1mol-1 or 8.314J K-1mol-1)
 Volume of one mole of an ideal gas at STP
 22.4 L
 Mole fraction, Χa
 Number of moles of gas a / total moles of the sample
 Partial Pressure, Pa
 Pa=XaPtotal
 Dalton’s Law
 The total pressure exerted by a gaseous mixture is the sum of the partial pressures of each of its gases.
 Average translational KE
 KE=3/2 RT
 Graham’s Law
 v1/v2=√m2/√m1
 Effusion
 Spreading of a gas from high pressure to low pressure through a pinhole.
 Diffusion
 Spreading of one gas into another gas or into empty space.
 Effusion Rate
 effusion rate1/effusion rate2 = √M2/√M1
 Real gases deviate from Ideal gases at:
 High pressure and Low Temperature
 Arrhenious Equation for rate constant, k, of a reaction
 k=Ae-Ea/RT
 Overall Reaction Order
 Sum of all the orders of each respective reactant.
 Rate determining step
 The rate of the slowest elementary step that determines the overall reaction.
 Slowest step is the first step
 The rate law can be derived directly from this step and no other. Ex: 1. NO2+NO2–>NO3+NO (slow) 2. NO3+CO–>NO2+CO2 (fast) rate = k[NO2]2
 Slowest step is other than the first step
 The slow step is still rate determining but setps prior to the slow step will contribute to the rate determing step. Ex: 1. NO+Br2–>NOBr2 (fast) 2. NOBr2+NO–>2NOBr (slow) rate = k[NOBr2][NO]
 mass = moles x MW
 Equilibrium
 Rate of the forward equals the reverse. This is the point of greatest entropy.
 aA+bB–>cC+dD The Law of Mass Action
 K=[C]c[D]d/[A]a[B]b   K is the equilibrium constant Let us write you a custom essay sample on MCAT General Chemistry Review 2 For Only \$13.90/page ORDER NOW
 Reaction Quotient, Q
 Q=[C]c[D]d/[A]a[B]b Q always changes towards K. Q = K, Equilibrium Q>K, leftward shift Q
 Le Chatlelier’s Principle
 When a system at equilibrium is stressed, the sstem will shift in a direction to reduce the stress. 1)Adding/removing reactants/products 2)Changing the pressure in the system 3) heating/cooling
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