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22 Cards in this Set
- Front
- Back
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Clapeyron's equation?
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p*V=n*R*T
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What type of exchange can occur between a system and the surrounding?
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-Energy exchange
-Matter |
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Define:
-Isolated system -Closed system -Open system |
-No exchange of matter or energy
-No exchange of matter but some exchange of energy -Exchange of both matter and energy |
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The properties of a state can be divided into...?
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Extensive parameters:
-Depends on the amount of substance present -Are additive Intensive parameters: -Do not depend on the amount of substance present -Are not additive |
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What forms may the exchange of energy take?
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-Heat
-Work |
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Heat flowing into a system is?
Heat flowing out of a system is? |
Positive
Negative |
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Define:
-Positive work. -Negative work. |
-Work that is done on the system by the surroundings: energy in the system is increased.
-Work that is done by the system on the surroundings: energy in the system is decreased. |
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Thermal equilibrium?
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No heat flow between two objects.
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Isobaric process?
Isochoric -"- ? Isothermal -"- ? Adiabatic -"- ? Cyclic -"- ? |
Constant pressure.
Constant volume. Constant temperature. Q=0, Exchange of energy through heat does not occur. Initial state = final state. |
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The 0'th law of thermodynamics?
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When two systems are in thermal equilibrium with a third body, they are also in thermal equilibrium with each other.
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The first law of thermodynamics?
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The change in the internal energy (ΔU) of a closed thermodynamic system is equal to the sum of the amount of heat (Q) energy supplied to the system and the work (W) done on the system.
ΔU=W+Q |
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Q>0 if?
Q<0 if? W>0 if? W<0 if? |
If heat flows into the system.
If heat flows out of the system. If work is done on the system. If work is done by the system. |
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The second law of thermodynamics?
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The total entropy of any isolated thermodynamic system tends to increase over time, approaching a maximum value.
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Heat resulting from chemical reactions in isobaric conditions equals the change in...?
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Enthalpy.
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ΔH<0 or ΔU<0?
ΔH>0 or ΔU>0? |
Exothermic process
Endothermic process |
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State the definition of enthalpy as an equation.
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H=U+pV
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Calculate the change in internal energy of 1 kg of water during boiling (at 100 C). The heat of vaporization is ΔH=2.26*10^6 J/kg. The desnity of saturated vapour at 100 C is 0.60 kg/m^3.
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ΔU=ΔH-pΔV
V(vapour)= mass/density = 1/0.6=1.67m^3 V(liquid)= 1 liter =0.001 m^3 ΔU=2.26*10^6-1013hPa*(1.67-0.001)= 2.09*10^6 J |
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Define ΔF (change in free energy).
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The maximal work that can be done by a system at constant temperature.
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Define ΔG (change in Gibbs free energy).
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The maximal (non-volume) work that can be done by a system at constant temperature and constant pressure.
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Exergonic reactions
What is the sign of ΔG? Do these reactions proceed spontaneously? |
-Negative
-Yes |
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Endergonic reactions
What is the sign of ΔG? Do these reactions proceed spontaneously? |
-Positive
-No |
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How can we make unfavourable reactions proceed?
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By favourable reactions.
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