Term
| Factors that affect the rate of reaction |
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Definition
| Catalysts, Medium, Temperature, Concentration of Reactants |
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Definition
| Catalysts are in the same phase as the reactant |
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| Catalysts are in a different phase from the reactants |
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Definition
| is the heat absorbed or evolved by a system at constant pressure |
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Definition
| no volume, no attractions or repulsions, ave KE is proportional to abs temp, elastic collisions, continuous random motion |
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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 |
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Definition
| the flow of gas particles under pressure from one compartment to another through a small opening. isothermal. r1/r2 = (mr2/mr1)^1/2 |
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Definition
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Definition
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Definition
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| Ideal Gas Equation and Encompassing Gas Eqtn |
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Definition
PV = nRT
P1V1/T1 = P2V2/T2 |
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Definition
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Definition
273.15K. 1 atm amd 22.4L/mol
Kinetics |
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Term
Standard Conditions
State functions |
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Definition
293.15K and 1 atm
Enthalpy, Entropy, Gibb's free energy |
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Term
| Ideal gas behaviour - exception |
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Definition
| seen at low pressure and high temperature. Exception = high pressure and low temperature bc molecular volume and intermolecular attraction become important |
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Term
| Dalton's Law of Partial Pressure |
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Definition
| Pa = XaPt where X = mole fraction & Pt = total pressure |
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Definition
| Xa = na (moles of A) /nt (total moles) |
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Definition
| is the speed which corresponds to the ave. KE per particle. Urms = (3RT/mr)^1/2 |
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