5046709
Beschreibung
Karteikarten von Jonas Schlicht, aktualisiert more than 1 year ago
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Erstellt von Jonas Schlicht
vor mehr als 8 Jahre
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| Frage | Antworten |
| Absolute (Kelvin) Temperature Scale | - lowest possible T = 0K - T(K) = t(°C) + 273 |
| Average random kinetic energy of molecules | average KE of a substance is proportional to the absolute T of a substance: 0.5mv2 = 2/3kT (k= Boltzmann constant) |
| Internal Energy (U) | total random KE of the molecules of a system + total intermolecular potential (thermal) energy |
| Intermolecular Forces | - are electromagnetic forces between any two molecules, - heating increases intermolecular potential energy, - ideal gases have no intermolecular forces |
| Heat, Q | 'Energy in Transit' - energy that is transferred form one body to another due to a difference in T |
| Direction of Energy flow | Heat is always transferred from a higher T region to a lower one. |
| Thermal Equilibrium | two bodies are at the same T & no further energy transfer |
| Ideal gas | - theoretical model - no intermolecular forces/potential energies - obeys equation pV=nRT at all P,V,T - real gases sometimes and roughly |
| mole | S.I. unit for quantity 1 mole = 6.02x10^23 = Avogadros constant |
| molar mass | mass of 1 mole in grams |
| Specific heat capacity, c | energy required to change T of a unit mass by 1°C/1K |
| Specific Latent Heat, L | energy required to change the phase of a unit mass at CONSTANT TEMP. |
| Change of phase | occurs at specific, constant temperature |
| Pressure | normal force per unit area: P=Fcosθ/A in Pa |
| Ideal gases | Assumptions: - hard spheres of negligible volume - collisions are elastic - short collisions - only forces between them during contact - random movement at various speeds - obey laws of mechanics |
| Real gases | - unlike ideal gases can liquify and solidify - always intermolecular forces - best approximation to ideal gas at low density (large volume, low pressure, moderate temperature) |
| Boiling | - boiling: specific T and molecules leave from anywhere in the liquid - evaporating: any T and surface molecules only (increase T or surface area to increase evaporation) - faster molecules escape; slower left behind; average speed/KE decreases; temperature decreases |
| Ideal gas law | pV=nRT |
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