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Premed95 > Chem4 - Thermodynamics > Flashcards

Chem4 - Thermodynamics Flashcards

1
Q

what is an extensive property?

A

proportional to system size (volume, mols)

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2
Q

what is an intensive property?

A

unrelated to system size (pressure, temperature)

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3
Q

what is the actual definition of temperature?

A

measure of amount of molecular movement

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4
Q

what is boltzmann’s constant(k)?

A

1.38e-23 JK-1(k)

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5
Q

what is the equation for average kinetic energy per molecule in any fluid?

A

KE=3/2kT(k is boltzman constant, T is temp in kelvin)

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6
Q

what is the equation for average KE per mol of molecule in a fluid?

A

KE=3/2RT

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7
Q

how do you convert from Celsius to Kelvin?

A

add 273 to celsius

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8
Q

what is a closed system?

A

can transfer energy but not mass

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9
Q

what is an isolated system?

A

cannot transfer energy or mass

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10
Q

what is a state function?

A

describes the state of a system in a path independent manner

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11
Q

what is internal energy?

A

collective energy of molecules measured microscopically

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12
Q

what is heat (q)?

A

describes spontaneous transfer of energy from warm to cold body

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13
Q

what is the zeroth law of thermodynamics?

A

states that temperature exists

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14
Q

what is conduction?

A

transfer of heat(thermal energy) via collisions and requires physical contact

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15
Q

what is convection?

A

thermal energy tansfer in a liquid (think air/ocean currents)

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16
Q

what is radiation?

A

thermal energy transfer using EM waves (white hot metal radiating heat)

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17
Q

what is Work (w)?

A

any energy transfer that isn’t heat

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18
Q

what is PV work?

A

work done by changes in pressure or volume

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19
Q

what is the equation for PV work?

A

w=-PΔV

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20
Q

PV work takes place when

A

gas expands against a force

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21
Q

what is the first law of thermodynamics?

A

energy is constant in a systemΔE=q+w

22
Q

what is the equation for enthalpy?

A

ΔH=ΔU+PΔV

23
Q

if only PV work is performed

A

ΔH=qenthalpy change=heat transferred into system

24
Q

what is standard state?

A

reference form for a substance at temperature T & pressure of 1 bar

25
Q

what is standard enthalpy of formation?

A

reaction that produces 1 mol of a compound from its raw elements in their standard states

26
Q

to calculate standard enthalpy of formation (ΔHoreaction)

A

, subtractΔH reactants fromΔHproducts

27
Q

what is the enthalpy change for an endothermic reaction?

A

positive , ΔH+

28
Q

what is the enthalpy change for an exothermic reaction?

A

negative, -ΔH

29
Q

breaking bonds ___ energy

A

consumes, + delta H

30
Q

forming bonds ____ energy

A

releases, -delta H

31
Q

what is entropy(s)

A

tendency for disorder

32
Q

what is the 2nd law of thermodynamics?

A

entropy of the universe will never decrease

33
Q

is entropy a state function?

A

yes, path does not matter.

34
Q

what is the equation for gibb’s free energy?

A

ΔG=ΔH-TΔS

35
Q

what is delta G of an endergonic reaction?

A

positiveΔG

36
Q

what is delta G ofan exergonic reaction?

A

NAME?

37
Q

ifΔH is negative andΔS is positive

A

always spontaneous

38
Q

ifΔH is positive,ΔS is negative

A

never spontaneous

39
Q

if bothΔH andΔS have the same sign

A

spontaneity depends on temperature

40
Q

what is hess’ law?

A

sum of each enthalpy change is equal to the total enthalpy change(adding up enthalpy changes, calculating with molar amounts)

41
Q

what is the actual definition for chemical equilibrium?

A

the rates of the forward and backward reaction rates are equal

42
Q

what is the equilibrium constant?

A

helps determine relative amounts of each substance at equilibrium

43
Q

what role do pure substances play in calculating the equilibrium constant?

A

none, they are given a value of 1 and do not contribue

44
Q

what is the reaction quotient?

A

identical to k except it does not represent the reaction at equilibrium

45
Q

if Q=K

A

reaction is at equilibrium

46
Q

if Q>K

A

reaction shifts to increase reactants(reverse rate is greater)

47
Q

if Q<K

A

reaction shifts to increase products(forward rate increases)

48
Q

what are the equations for free energy?

A

ΔG=ΔGo+RTln(Q)ΔGo=-RTln(K)

49
Q

if a reaction has K>1

A

reaction is spontaneous under the temp required to derive that value

50
Q

a second order reaction involves only __ reactant molecules

A

2

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