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BMAT Chemistry > THERMODYNAMICS > Flashcards

THERMODYNAMICS Flashcards

1
Q

what is thermodynamics

A

the study of energy and its relationship to chemical systems

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2
Q

what two things are needed for a thermodynamic system

A

a system and its surroundings

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3
Q

define system

A

object that experiences a thermodynamic transformation.

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4
Q

define surroundings

A

Any part of the universe that is in direct contact with the system is its surroundings

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5
Q

what are the three types of system

A

open, closed, and isolated

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6
Q

what occurs in an open system

A

heat transfer
mass transfer

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7
Q

what occurs in a closed system

A

heat transfer
no mass transfer

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8
Q

what occurs in an isolated system

A

no heat or mass transfer

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9
Q

define work in a thermodynamic context

A

any energy transfer that is not heat

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10
Q

what is internal energy also called and how can we calculate this simply

A

average total mechanical energy (kinetic + potential) of the particles that make up the system.

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11
Q

what are the three types of heat transfer

A

conduction, convection, and radiation

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12
Q

what is heat

A

transfer of energy from a warmer body to a cooler body

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13
Q

how does conduction carry out thermal energy transfer

A

thermal energy transfer via molecular collisions, requires direct physical contact

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14
Q

what is required for the particles in conduction to transfer thermal energy

A

direct physical contact

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15
Q

how do molecule collisions in conduction carry out thermal energy transfer

A

higher energy molecules of one system transferring some of their energy to the lower energy molecules of the other system via molecular collisions

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16
Q

what is convection

A

thermal energy transfer via fluid movements

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17
Q

how does convection transfer thermal energy

A

Warm fluid moves in the direction of cooler fluid due to differences in pressure or density

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18
Q

what is radiation

A

Radiation is thermal energy transfer via electromagnetic waves

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19
Q

what does the first law of thermodynamics state

A

energy of the system and its surroundings is always conserved

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20
Q

what is Q

A

Q = Quantity of heat supplied to the system by its surroundings

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21
Q

What is W

A

W = Net work done by the system

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22
Q

what happens in the change in internal energy equation when work is done on the system

A

Work done on system = + W

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23
Q

what happens in the change in internal energy equation when work is done by the system

A

Work done by system = - W

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24
Q

what happens in the change in internal energy equation when heat is added to a system

A

Heat added to system = +Q

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25
Q

what happens in the change in internal energy equation when heat is given off by a system

A
  • Heat given off by system = -Q
26
Q

how do you calculate change in internal energy

A

Change in U = +/-Q +/- W

27
Q

what is the second law of thermodynamics trying to prove

A

heat cannot be completely changed to work in a cycle-like process

28
Q

what does the second law of thermodynamics show about heat transfer direction

A

allows for the determination of the preferred direction of a given transformation – for example, we know that heat flows from a hot source to a cold source

29
Q

what is the symbol and unit for internal energy

A

U

Joule

30
Q

what is the symbol and unit for temperature

A

T

Kelvin

31
Q

what is the symbol and unit for pressure

A

P

Pascal

32
Q

what is the symbol and unit for volume

A

V

m^3

33
Q

what is the symbol and unit for enthalpy

A

H

kJ mol-1

34
Q

what is the symbol and unit for entropy

A

S

JK mol^-1 (joules per kelvin)

35
Q

what is the symbol and unit for gibbs free energy

A

G

kJ mol-1

36
Q

what is internal energy

A

collective energy of molecules

37
Q

in a system with constant volume and no work what is the internal energy the same as

A

heat

38
Q

for internal energy to be equated to heat, what is the condition

A
  1. constant volume
  2. no work done
39
Q

what is temperature an example of

A

thermodynamic property

40
Q

in fluid, temperature is directly proportional to what

A

the translational kinetic energy of its molecules

41
Q

in gas, what happens if the translation energy per mole of gas increases

A

greater the temperature

greater pressure

42
Q

how do you convert from Celsius to Kelvin

A

0 celsius = 273.15K

+ 273.15 to whatever required

then every 1kelvin = 1Celsius

43
Q

convert 30 celsius water to kelvin

A

273.15 + 30
= 303.15 kelvin

44
Q

if a pot of water is at 303.15 and you increase it by 1 celsius, what is the water temperature in kelvin

A

304.15 kelvin

31°C

45
Q

what is enthalpy’s basic law

A

H = internal energy + (pressure x volume)

46
Q

what is standard enthalpy of formation

A

enthalpy to make one mole of compound from elements

47
Q

what is enthalpy used to approximate

A

heat

48
Q

what is the equation for change in enthalpy

A

Products - reactants

49
Q

what does hess’ law state

A

when adding reactions, their enthalpies can be added because enthalpy is a state function

50
Q

what is an exothermic value in enthalpy

A

-ΔH

enthalpy of products is less than enthalpy of reactants

51
Q

what is an endothermic value in enthalpy

A

+ΔH

enthalpy of products is more than enthalpy of reactants

52
Q

what is entropy

A

degree of disorder in a system

53
Q

what state of matter has the highest entropy

A

gas

54
Q

how does entropy increase

A

solid to a liquid to a gas

55
Q

why does gas have a higher entropy than water

A

gas molecules exhibit an increased random motion of movement

56
Q

what does gibbs free energy determine

A

if a reaction is spontaneous or not, or if the reaction is at equilibrium

57
Q

what is the equation for gibbs free energy

A

∆G = ΔH - (T x ΔS)

58
Q

what happens if ∆G is less than 0 [at constant pressure]

A

spontaneous

59
Q

what happens if ∆G is 0

A

in a state of equilibrium

60
Q

what happens if ∆G is more than 0 [at constant pressure]

A

not spontaneous

BMAT Chemistry (7 decks)

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