Thermochemistry
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| System | A specific amount of matter that is being studied
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| Surroundings | Everything outside of the system
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| Open system | A system that can transfer energy and matter to its surroundings
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| Closed system | A system that can transfer energy, but not matter, to its surroundings
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| Isolated system | A system that does not transfer energy or matter to its surroundings
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| Work | The energy required to move and object over some distance
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| Equation for work | w = (F)(d)
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| Force due to gravity | F = (m)(g)
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| Gravitational potential energy | w = (m)(g)(h)
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| State function | The value depends only on the present state of the system, not the path it took to get there
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| Endothermic | Heat flows into the system from its surroundings (+ΔE)(+ΔH)
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| Exothermic | Heat flows from the system into its surroundings (-ΔE)(-ΔH)
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| Internal energy (E) | The sum of all kinetic and potential energies of the components of the system
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| ΔE | Change in internal energy
= (initial E) - (final E)
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| Relating ΔE to heat and work | ΔE = q + w
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| Enthalpy (H) | A thermodynamic function used to account for the heat flow during a constant pressure process
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| Equation for enthalpy | H = E + PV
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| Pressure-volume work | Work performed by expansion of a gas against a resisting pressure
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| P-V work when pressure is constant | w = –P ΔV
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| Calorimeter | A device used to measure heat flow
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| Heat capacity (C) | The amount of heat required to raise the temperature of a sample of matter by 1 K
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| Molar heat capacity (Cm) | The amount of heat required to raise the temperature of one mole of a substance by 1 K
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| Specific heat (Cs) | The amount of heat required to raise the temperature of one gram of a substance by 1 K
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| Equation for specific heat | Cs = (q)/(mΔT)
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| Equation for heat gain or loss | q = m x Cs x ΔT
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