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| pressure equals force divided by the area p=F/A |
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| in science it is always measured in Kelvin (Celsius + 273.15 = Kelvin) |
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| Equation of state for perfect gases |
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| pV=nRT, at constant temperature boyles law p=1/V |
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| When two bodies in contact have the same temperature and there is no net flow of energery between them |
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| Each constant temperature curve on a graph of pressure versus inverse of volume (p = 1/V) |
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| represent change in atmospheric pressure on a weather map, in increments of 4 mbar or 400pa |
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| Z=Vm/Vm(perfect) // Vm = V/n = RT/p (this is molar volume equation volume divided by number of moles in that volume or R x temp divided by pressure) Z=pVm/RT |
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| Van der Waals equation of state |
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| p=(nRT/(V-nb))-a(n/V)^2 p=(RT/Vm-b)-a/Vm^2 |
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| potential energy vs particle separation |
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| potential energy = mass x gravity x height gravity=9.81 m s^-2 Coulomb potential energy = Q1Q2/4 x pi x r |
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| attractive and repulsive forces |
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| The temperature at which a gaseous state transforms continuously into the condensed state and at no stage is there a visible surface between the two states of matter (a gas cannont be condensed to a liquid by the application of pressure unless the temperature is below the critical temperature) vapour is the gaseous phase of a substance below its critical temperature |
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| critical constants Tc,pc,Vc |
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Definition
| All three of these temperature pressure and volume make up the critical constants |
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| can exchange energy but not matter with its surroundings |
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| a system does work when it causes motion against an opposing force w=mgh (mass x gravity x height) expansion work = p(external) x hA = p(external) x dV Work=-nRTln(Vfinal/Vinitial) Work=pdV (pressure x delta volume) |
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| the process of transferring energy as a result of a temperature difference between the system and its surrounding q heat capacity c=q/dT or q=c x dT |
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| internal energy (U) = heat + work heat (q)= |
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| Walls/boundaries that permit heating as a mode of transfer of energy |
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| a process in a system that releases energy as heat |
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| first law of thermodynamics |
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| The internal energy of an isolated system is constant |
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| expansion work against constant pressure |
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| expansion work for isothermal reversible process |
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| hydrostatic pressure = denstiy x height x gravity density = mass/volume |
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| Equation of state for real gases |
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| Walls/boundaries that do not permit heating even though there is a difference in temperature on both sides |
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| a process in a system that absorbs energy as heat |
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| can exchange both energy and matter with its surroundings |
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| can exchange neither matter nor energy with its surroundings |
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| xj = nj/n partial pressure = amount of j molecules in the mixture divided by the total amount |
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