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Definition
study of energy transfer and energy transformation
energy absorbed/released |
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| ability to do work or to supply heat |
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| when an object is moved by force over a distance |
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| difference in temperature when applied to energy |
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| what are the two ways energy is transferred |
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Definition
heat and work
objects DON'T CONTAIN HEAT OR WORK!!
its internal energy that does |
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| everything needs to be stable so it goes to kinetic energy |
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| chemical potential energy |
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Definition
interaction between particles in an atom
constant randomn motion so they have a kinetic energy>thermal energy
average KE is proportional to temp in gas |
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Definition
something is defined as system and everything else in surroundings
system is usually reactants and products
energy transferred between both |
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Definition
sum of potential and kinetic energy
change U= U final- U inital which is q+w
first law of thermodynamics>no energy lost |
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| when heat or work goes into system |
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Definition
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| when heat or work goes out of system |
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Definition
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| systems absorbs heat so it is positive; energy converted to chemical potential energy |
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| system releases heat so it is negative; energy converted to thermal |
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| internal energy is what kind of system |
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Definition
| state function; unique value once the conditions of system have been defined |
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| geat and work are what kinds of system |
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Definition
| no state functions bc they depend on the system |
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Definition
| heat transfer at constant temperature |
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| heat reaction (q rxn) with constant volume |
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Definition
qv would just equal Q +W
no work is actually done so all energy is heat |
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| heat reaction (q rxn) with constant pressure |
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Definition
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| U +PV; heat transfer at constant pressure |
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| relationship with enthalpy and internal energy |
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Definition
| changes in both equals each other |
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Term
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Definition
| measurement of quantity of heat |
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| heat capacity (C) and equation |
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Definition
heat required to change the temperature of a system by 1 degree c;
c=q/change in T |
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Definition
| heat required to change the tempeature of system by 1 degree over 1 mole |
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Definition
| heat capacity of 1 gram of sample |
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Term
| heat equation with specific heat |
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Definition
q= m (specific heat) (change in T)
MCAT |
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| same as change H which is q+w; constant pressure |
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Definition
constant volume; can be change in U + p change in V; but normally just
q+W |
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Definition
| enthaply is state function so no matter the order or steps the energy with still be the same |
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Definition
reference for thermo.
1 atm, 1 M, 25 degree C, |
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Definition
| enthaply change when all reactants and products are in their standard states |
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