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PMP102 > Concepts of Thermodynamics -ALL NOTES > Flashcards

Concepts of Thermodynamics -ALL NOTES Flashcards

1
Q

What is potential energy?

A

-Stored energy

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2
Q

What are examples of potential energy?

A

-Raised weight, stretched rubber band, charged battery

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3
Q

What are examples of kinetic energy?

A

-Boiling water, desk lamp, buzzing bee

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4
Q

What is kinetic energy?

A

-Energy of moving objects

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5
Q

What is thermodynamics?

A

-The science of energy interconversion

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6
Q

What is an isolated system?

A

-An isolated system cannot exchange energy or matter with its surroundings

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7
Q

What is a closed system?

A

-A system where mass cannot transfer but energy can

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8
Q

What is an open system?

A

-An open system can exchange both energy and matter with its surroundings

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9
Q

What is the zeroth law of thermodynamics?

A

-If two systems are in thermal equilibrium with a third system the two original systems are in thermal equilibrium with each other

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10
Q

What is the first law of thermodynamics?

A

-Energy can not be created or destroyed- only transformed from one form to another

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11
Q

What is the equation for the conservation energy?

A

-deltaU= Q-W

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12
Q

What does it mean if the Q is positive in the first law of thermodynamics ?

A

-Heat is added to the system so is an endothermic process

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13
Q

What does it mean if the Q is negative in the first law of thermodynamics ?

A

-Heat is released from the system so exothermic process

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14
Q

What is an SI unit?

A

-International System of Units equal to a joule or cal/kcal

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15
Q

What is 1 calorie?

A

-Heat needed to raise the temperature of 1 gram of water 1oc at standard pressure?

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16
Q

What is heat capacity?

A

-Amount of heat required to raise a substances temperature by 1 kelvin

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17
Q

What is specific heat capacity?

A

-Amount of heat required to raise 1 gram of a substance by 1 kelvin

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18
Q

What is the symbol for heat capacity?

A

-C

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19
Q

What is the symbol for specific heat capacity ?

A

-Cs

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20
Q

What is enthalpy?

A

-The measurement of energy in a thermodynamic system

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21
Q

What is the equation for enthalpy?

A

-deltaH = deltaE + delta(PV)

22
Q

What can you assume about enthalpy equation in cells?

A
23
Q

What happens to enthalpy in an endothermic process?

A

-

24
Q

What happens to enthalpy in an exothermic process?

A

-

25
Q

What is the second law of thermodynamics ?

A

-The universe is always moving towards maximum disorder

26
Q

What is entropy ?

A

-Measure of disorder

27
Q

What is the third law of thermodynamics?

A

-At absolute zero (0K) the entropy of a perfect, crystalline substance is zero

28
Q

Why does entropy equal 0 at absolute zero?

A

-There is a perfect crystalline structure so all vibrations and atomic movements stop

29
Q

What temperature is absolute zero in degrees Celsius?

A

-273.15 oc

30
Q

What does G stand for?

A

-Gibbs free energy

31
Q

What is Gibbs free energy?

A

-Energy available to do work and the spontaneity of a reaction

32
Q

What does H stand for?

A

-Enthalpy (KJ mol-1)

33
Q

If delta G is negative is the reaction spontaneous?

A

-Yes, in a forward reaction only

34
Q

If delta G is zero is the reaction spontaneous ?

A

-Yes, at equilibrium, can proceed in either direction

35
Q

If delta G is positive, is the reaction spontaneous ?

A

-No, unless coupled with an energetically favourable reaction

36
Q

What is free energy of formation?

A

-The free energy change which results from 1 mol of substance prepared from its elements at standard temperature and pressure

37
Q

How do you calculate free energy of formation?

A

-Delta G of formation of products minus delta G formation of reactants

38
Q

What is the standard enthalpy change of a reaction?

A

-The heat transferred by a chemical reaction or process under standard conditions

39
Q

What is bond dissociation energy?

A

-The enthalpy change per mol in the gas phase when a bond is broken

40
Q

What does D stand for?

A

-Bond dissociation enthalpy

41
Q

Is bond dissociation enthalpy positive or negative?

A

-Positive as bond breaking is an endothermic process

42
Q

What is the standard entropy change of a reaction?

A

-The difference in standard entropy between the products and reactants of a system ubnder standard conditions

43
Q

If a reaction is at equilibrium, what happens at E on the graph?

A

-G rises if the reaction proceeds in either direction

44
Q

What does K stand for?

A

-The composition of a reaction mixture when it comes to equilibrium

45
Q

What are the features of using K?

A

-Used in heterogenous reactions, must be associated with a specific temperature and equation of the reaction

46
Q

What is Q?

A

-Measures the composition of the reaction mixture as the reaction progresses, not at equilibrium

47
Q

If K is more than Q, what reaction proceeds?

A

-Forward

48
Q

If K is less than Q what reaction proceeds?

A

-Reverse

49
Q

If K=Q what reaction proceeds?

A

-both-at equilibrium

50
Q

What is Le Chatelier’s principle ?

A

-When a change is made to a system in dynamic equilibrium, the system responds to minimise the effect of the change

PMP102 (20 decks)

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