thermodynamics Flashcards

1
Q

thermodynamics

A

study of heat

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1
Q

heat

A

energy transfer through temperature

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2
Q

temperature

A

average kinetic energy of the motions of a molecule

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3
Q

temperature of ideal gas equation

A

KE= .5mv^2(rms)
v is sqrt of v^2 rms is sqrt(3RT/M)
- t is temp (k)
R is ideal gas constant
M is molar mass

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4
Q

kinetic energy and heat equation

A

KE= 3/2 t*(r/m)
1. kinetic energy is proportional to temperature
2. details of model apply to ideal gases

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5
Q

what is kinetic energy measured as

A

temperature in kelvin

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6
Q

system

A

subset of the universe that is being modeled

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7
Q

internal thermodynamic equillibrium

A

no macroscopic transfers of energy are taking place

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8
Q

open systems

A

exchange matter and energy with sorroundings
- human body is an open system

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9
Q

closed system

A

exchange energy with sorroundings but not matter
- example is a capped test tube

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10
Q

isolated system

A

canNOT exchange matter or energy with sorroundings
- no true insulators in nature

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11
Q

state functions

A

variables like energy, temperature, entropy, gibbs free energy and enthalpy
- pressure, volume, density
- describe state of system without describing how it got there

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12
Q

path functions

A

heat and work
- describe how you got from one equillibrium to another state

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13
Q

zeroth law (thermodynamics)

A

if system A is in equilibrium with system B and C then systems B and C are in thermal equillibrium with each other
- temp

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14
Q

Fahrenheit scale

A

32 F is freezing
bp is 212F
body temp is 98.6

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15
Q

celcius scale

A

body: 37 C
freeze 0 C

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16
Q

conversion from celcius to Farenheit

A

(F-32)*5/9

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17
Q

conversion from C to F at high temp

A

9/5

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18
Q

kelvin

A

0 K= 273 C
K- 273 = C

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19
Q

first law of thermodynamics

A

for closed systems: the total energy change of a system ΔU equals the transfer of energy into the system via heat minus the work performed by the system on its sorroundings
ΔU= Q- W
- comtribition of heat and work

20
Q

work being added to a system

21
Q

work being taken from a system

22
Q

+Δ U

A

energy is being added to the system

23
Q
  • ΔU
A

energy is being removed from the system

24
+ΔQ
heat is flowing into the system
25
second law of thermodynamics
if two objects are in contact and not in thermal equilibrium, heat will be transferred from high temperature to low temperature - the entropy of an isolated system will increase over time
26
entropy
measure of disorder connected to energy , how much energy is available to do work
27
boltzmann's formula
S = Kb*lnW - s is entropy - kb is constant - w is number of microstates of an observable substance (degrees of freedom)
28
what does an increase in degrees of freedom mean in terms of entropy
increase df increase entropy
29
order the amount of entropy from highest to lowest liquids, solids, gas
solid --> liquid --> gas
30
entropy and work
Δs = q/T
31
can entropy be decreased
yes, but it takes considerable energy (if you break a glass bottle and it shatters it is not easy to piece together)
32
major entropy concepts for MCAT
1. energy will flow from hot to cold items 2. entropy inevitably increases in a true isolated system
33
third law of thermodynamics
at absolute o (0 Kelvin) a crystal structure has an entropy of 0
34
t/f: heat and temperature are different things
TRUE heat is a transfer of energy, temperature is average kinetic energy
35
units of heat
j, calories
36
heat transfer methods
1. conduction 2. convection 3. radiation
37
conduction
two objects with different temperatures touch and heat transfers from hot to cold
38
convection
heat transfer between two objects due to the circulation of fluid - thermal differences due to the densities of fluids
39
radiation
no direct contact - heat transfer via electromagnetic waves
40
thermal expansion
idea that as temperature increases, the object expands
41
exception to thermal expansion
ice is less dense than water and reaches peak density at 4C
42
solid expansion equation
ΔL= alphaL *ΔT - measure change in L - alpha is coefficient of thermal expansion that is specific to substance
43
liquid expansion equation
ΔV = alphav*ΔT
44
ideal gas equation
PV=nRT
45
isothermic system
temp constant on a pressure volume graph
46
adiabatic system
no heat or matter is transferred between a system and its sorroundings - constant entropy - steeper slope than isothermic
47
isobaric
constant presssure