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27 Cards in this Set
- Front
- Back
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1st law of Thermodynamics
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Energy of the universe is constant;
Energy can never be created or destroyed |
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2nd law of Thermodynamics
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System spontaneously move toward disorder(high entropy)
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ΔE:?
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ΔE= q + E
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w= -pΔV
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+w = V is -
-w = V is + |
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Locked piston
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ΔE = q
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Unlocked piston: When heat piston
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Volume increases
Work is - PE increases so ΔE decreases " Expanding gases cool" |
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Unlocked piston: Put weight on piston
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Work is +
Temp increases "compressed gases warm" |
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Isobaric
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Pressure constant
area= work done by gas |
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Isochoric
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Volume constant
Area= 0 so work= 0 |
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Isothermal
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Temp constant
ΔE=0 so q=-w |
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Adiabatic
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no heat transfer
q=0 ΔE=w "perfectly insulated system" |
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Entropy
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Amount of disorder
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Increasing entropy means:
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1) Phase change
2) Increasing # of moles of gas dissolved; the side with the more mol of gas has more entropy |
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Enthalpy
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amount of heat gained or lost when bonds are formed or broken
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Bond breaking
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requires energy
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Bond forming
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releases energy
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(-)ΔH
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exothermic
heat is product product have stronger bond that the reactant |
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(+)ΔH
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endothermic
heat is reactant reactant have stronger bonds |
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Hf=0 when?
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when elements are in their natural state
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ΔG
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Gibbs free energy
Energy evolved or absorbed as the rxn goes from rxn to product |
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(-)ΔG
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product have less energy
more stable spontaneous exergonic(energy is given off) |
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(+)ΔG
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Product have more energy
less stable nonspontaneous endergonic |
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ΔG=0
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prod and reac have same energy
rxn is @ equilibrium |
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Low temperature
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ΔH dominated
if ΔH and ΔS are both (-):spon |
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High temperature
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ΔS dominates
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Kinetics
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rates, activation Energy, catalyst, temp
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Thermodynamics
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ΔG, H, S, Equilibrium, Temperature
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