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Definition
| the system cannot exchange energy (heat and work) or matter with the surroundings; ie an insulated bomb calorimeter |
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Definition
| the system can exchange energy (heat and work) but not matter with the surroundings; a steam radiator |
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Definition
| the system can exchange both energy (heat and work) and matter with the surroundings; ie a pot of water |
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| first law of thermodynamics |
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Definition
deltaU = Q - W
Where U is the change in internal energy of the system, Q is heat added to the system and W is work done by the system |
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Definition
| process that keeps temperature constant which in turn means total internal energy of the system is constant; change in U is zero so Q = W (first law of thermodynamics) |
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Definition
| no heat is exchanged between the system and the environment; thus, the thermal energy of the system is constant throughout the process; Q = zero so deltaU = -W |
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Definition
| pressure is held constant; does not alter the first law of thermodynamics |
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Definition
| also isochoric, no change in volume; if the gas neither expands nor compresses, no work is performed meaning the first law simplifies to deltaU = Q |
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| What are standard conditions and what are they used for? |
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Definition
| Standard conditions are 25 C, 1 atm pressure and 1 M concentrations. They are used for kinetics, equilibrium and thermodynamics problems |
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Definition
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Definition
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Definition
| the transfer of energy from one substance to another as a result of their differences in temperature; represented by Q |
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| Equation to calculate the heat absorbed or released on a process |
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Definition
q = mc(deltaT)
q is heat
m is mass
c is specific heat
deltaT is change in temperature |
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Term
| Equation used to calculate the heat of a phase change |
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Definition
q = mL
q is heat
m is mass
L is latent heat which describes the enthalpy of an isothermal process |
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Definition
| a state function that is equal to the heat transferred in or out of the system at constant pressure |
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Definition
| enthalpy changes of reactions are additive |
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Definition
| the measure of the spontaneous dispersal of energy at a specific temperature, represented by 'S' |
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| second law of thermodynamics |
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Definition
| energy spontaneously disperses from being localized to becoming spread out if it is not hindered from doing so |
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Definition
| relates the temperature, enthalpy and entropy to determine spontaneity of a reaction |
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Definition
| a reaction that releases energy; spontaneous |
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Definition
| a reaction that absorbs energy; nonspontaneous |
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| equation that relates free energy and the equilibrium constant and the version used for reactions in progress |
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Definition
ΔGorxn = -RT ln Keq
R is the ideal gas constant
T is the temperature in kelvins
Keq is the equilibrium constant
ΔGrxn = ΔGorxn + RT lnQ =RT ln(Q/Keq)
Q is the reaction quotient |
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