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23 Cards in this Set
- Front
- Back
Heat
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thermal energy transferred between a system and its environment
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when does spontaneous heat transfer occur?
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between systems at different temperatures
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specific heat
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c
amount of E_th absorbed/liberated per unit mass of material per unit temperature change |
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c formula
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c = Q / m∆T in UoM cal / g C°
Q is calories of heat m is mass in g T is temp in C° |
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calorie
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Q required to raise 1 g water from 14.5 °C to 15.5 °C
1 cal = 4.186 J |
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BTU
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Q required to raise 1 lb water from 63 °F to 64 °F
1 BTU = 778 ft-lb |
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Given a sample heated in boiling water and then transferred to water in a calorimeter can, one can find the specific heat of the sample.
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Conservation of E says Q_s = Q_c + Q_w
s: sample, c: cup, w: water given c = Q / m∆T, rearrange to Q = cm∆T Sub the cm∆T for the Q's in the above equation, and then rearrange to solve for C_s C_s = (C_wM_w)(T_c - T_o) + (C_A*M_c(T_c - T_o) / (M_s ( T_B - T_c) where T_B = boiling, T_o = original temp, T_c = final temp |
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Latent Heat
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heat absorbed or liberated during a phase transition
∆T = 0 |
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L
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latent heat
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L_f
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latent heat of fusion
liquid ↔ solid |
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L_v
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latent heat of vaporization
liquid ↔ gas |
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Water & L
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L_f at 0 °C
L_v at 100 °C |
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L formula
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Q = mL_f,v
heat transfer = mass * Latent heat (of fusion or vaporization) |
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L_f,v - negative or positive?
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< 0 if going from a warmer state to a cooler state
> 0 if going from a cooler state to a warmer state |
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L values for water in cal / g
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L_f = 80 cal / g = 333 kJ / kg
L_v = 539 cal / g = 2260 kJ / kg |
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graph of temperature as a function of Q added to 1 g ice at -20 °C
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linear rise to 0°C
flat as it melts linear rise from 0°C to 100 °C flat as it vaporizes linear rise beyond 100 °C |
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plateaus of temp / Q graph represent...
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phase change
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sloped portions of temp / Q graph represent...
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changes in temperature of a substance with no associated phase change
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Sensible Heat
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Q absorbed or liberated with ∆T
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Q_s
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sensible heat
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Q_L
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latent heat aka heat of transformation
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Q & conservation of energy
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energy used to cool something = energy absorbed by the thing used to cool it
conversely energy used to warm something = energy liberated by the thing used to warm it |
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Q, conservation of energy, formula
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Q_absorbed = Q_liberated
think about whether something in an experiment is absorbing or liberating heat |