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S1 - Medicinal Chemistry > Thermodynamics > Flashcards

Thermodynamics Flashcards

1
Q

What is thermite ?

A
  • Metal powder and metal oxide
  • Exothermic reduction-oxidation (redox) reaction
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2
Q

Thermite equation

A
  • Fe2O3 + 2 Al → 2 Fe + Al2O3 + HEAT
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3
Q

What is thermodynamics ?

A
  • is the science of the relationship
    between heat and other forms of energy.
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4
Q

What is thermochemistry ?

A
  • is the study of the quantity of heat
    absorbed or evolved by chemical reactions
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5
Q

Radiant energy

A
  • comes from the sun and is earth’s
    primary energy source.
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6
Q

Thermal energy

A
  • is the energy associated with the
    random motion of atoms and molecules
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7
Q

Chemical energy

A
  • is the energy stored within the bonds of chemical substances
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8
Q

Nuclear energy

A
  • is the energy stored within the collection of neutrons and protons in the atom.
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9
Q

Potential energy

A
  • is the energy available by virtue of an object’s position
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10
Q

What is energy ?

A
  • The capacity to supply heat or do work.
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11
Q

Kinetic Energy (EK)

A
  • The energy of motion
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12
Q

Potential Energy (EP)

A
  • Stored energy
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13
Q

Thermal Energy

A
  • The kinetic energy of molecular motion,
    measured by finding the temperature of an object.
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14
Q

What is heat ?

A
  • The amount of thermal energy transferred from one object to another as the result of a temperature difference between the two
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15
Q

Law of Conservation of Energy

A
  • Energy cannot be created or destroyed; it can only be converted from one form to another.
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16
Q

First Law of Thermodynamics

A
  • Energy cannot be created or destroyed; it can only be converted from one form to another
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17
Q

What is an isolated system ?

A
  • can neither do work upon nor heat their
    surroundings
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18
Q

The internal energy of an isolated system is

A
  • constant
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19
Q

Change in energy equation

A

∆E = Efinal - Einitial

20
Q

What is an exothermic process ?

A
  • change (e.g. a chemical reaction) that releases heat
21
Q

What does a release of heat correspond to ?

A
  • decrease in enthalpy
22
Q

What is an endothermic process ?

A
  • a change (e.g. a chemical reaction) that requires (or absorbs) heat.
23
Q

What does an input of heat correspond to ?

A
  • an increase in enthalpy
24
Q

What is enthalpy ?

A
  • the measurement of energy in a thermodynamic
    system.
25
Q

What is an open system ?

A
  • Can exchange both matter and energy with the
    surroundings (e.g. open reaction flask, rocket engine)
26
Q

What is a closed system ?

A
  • Can exchange only energy with the surroundings (matter remains fixed) e.g. a sealed reaction flask.
27
Q

What is an isolated system ?

A
  • Can exchange neither energy nor matter with
    its surroundings (e.g. a thermos flask).
28
Q

What is state function ?

A
  • A function or property whose value depends
    only on the present state, or condition, of the system, not on the path used to arrive at that state.
29
Q

Equation for work ?

A
  • work = force x distance
30
Q

What is expansion work ?

A
  • Work done as the result of a volume change in the system.
  • Also called pressure-volume or PV work.
31
Q

Equation for ∆E

A

∆E = q + w

32
Q

Equation for q ?

A
  • q = ∆E + P∆V
33
Q

What is q ?

A
  • heat transferred
34
Q

Equation for w ?

A
  • -P∆V
35
Q

What is ∆ H ?

A
  • heat given off or absorbed during a reaction at constant pressure
36
Q

What is the pressure in a vacuum ?

A
  • 0 atm
37
Q

Thermodynamic Standard State

A
  • Most stable form of a substance at 1 atm pressure (po)
  • at a specified temperature, usually 25°C
  • 1M concentration for all substances in solution
38
Q

What is Hm ?

A
  • Standard Molar Enthalpy of a substance.
39
Q

What are phase transitions accompanied by ?

A
  • Most phase transitions are accompanied by a change in enthalpy
40
Q

Enthalpy of Fusion (∆Hfusion)

A
  • The amount of heat necessary to melt a substance without changing its temperature.
41
Q

Enthalpy of Vaporization (∆Hvap)

A
  • The amount of heat required to vaporize a substance without changing its temperature.
42
Q

Enthalpy of Sublimation (∆Hsubl)

A
  • The amount of heat required to convert a
    substance from a solid to a gas without going through a liquid phase.
43
Q

Is ∆ H negative or positive for endothermic reactions ?

A
  • positive
44
Q

What is the equation for ∆Hsubl ?

A
  • ∆Hsubl = ∆Hfusion + ∆Hvap
45
Q

Is ∆ H negative or positive for exothermic reactions ?

A
  • negative
46
Q

What happens if you reverse a reaction ?

A
  • the sign of ∆H changes

S1 - Medicinal Chemistry (11 decks)

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