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24 Cards in this Set
- Front
- Back
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Standard temperature and pressure (STP)
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0⁰ C and 1 atm
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Mean free path
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The distance traveled by a gas molecule between collisions
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Ideal gas law
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PV = nRT
R = 0.08206 L atm/ K^-1 mol^-1 R = 8.314 J K^-1 mol^-1 T in Kelvin |
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At STP one mole of any gas (behaving ideally) will occupy the
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standard molar volume of 22.4 liters
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Partial pressure
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Total pressure of a gaseous mixture times the mole fraction of the particular gas. Pₐ = αₐ P(total)
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Dalton's law
Total pressure exerted by a gaseous mixture is the sum of the partial pressures of each of its gases |
P(total) = P₁ + P₂ + P₃...
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Average translational kinetic energy
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KE(avg) = (3/2)RT
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Grahams law
Average speed of molecules of a pure gas is inversely proportional to the square root of the mass of the gas molecule |
(v₁/v₂) = √m₁ /√m₂
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Effusion
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The spreading of gas from high pressure to very low pressure (through a pinhole)
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Rates of effusion
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(effusion rate₁/ effusion rate₂) = √M₂ /√M₁
M = molecular weight |
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Diffusion
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The spreading of one gas into another gas or into empty space
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Real vs. Ideal
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V (real) > V (ideal)
P (real) < P (ideal) |
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Kinetics
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The rate of reaction as it moves toward equilibrium
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Thermodynamics
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The balance of reactants and products after they have achieved equilibrium
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Activation energy
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The threshold energy required in a collision to create new molecules
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Elementary reaction
Occurs in a single step Rate Law |
aA + bB → cC + dD
rate(forward) = kf [A]^α[B]^β α + β = overall order of the reaction α = a β = b |
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Intermediates
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Species that are products of one reaction and reactants of a later reaction in a reaction chain
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Kinetics
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The rate of reaction as it moves toward equilibrium
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Thermodynamics
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The balance of reactants and products after they have achieved equilibrium
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Activation energy
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The threshold energy required in a collision to create new molecules
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Elementary reaction
Occurs in a single step Rate Law |
aA + bB → cC + dD
rate(forward) = kf [A]^α[B]^β α + β = overall order of the reaction α = a β = b |
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Intermediates
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Species that are products of one reaction and reactants of a later reaction in a reaction chain
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Chemical equilibrium
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The forward reaction rate equals the reverse reaction rate
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Le Chatelier's principle
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When a system at equilibrium is stresses, the system will shift in a direction that will reduce stress
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