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AP Chemistry > Chapter 6: Thermochemistry > Flashcards

Chapter 6: Thermochemistry Flashcards

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1
Q

Energy

A

The capacity to do work or to produce heat

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2
Q

Law of Conservation of Energy

A

Energy can be converted from one form to another but can be neither created nor destroyed (The energy gained by the surroundings must be equal to the energy lost by the system.)

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3
Q

Potential energy

A

Energy due to position or composition

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4
Q

Kinetic energy

A

Energy due to the motion of the object and depends on the mass of the object and its velocity (KE = 1/2 x m x v^2)

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5
Q

Heat

A

The transfer of energy between two objects due to a temperature difference

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6
Q

Work

A

Force acting over a distance

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7
Q

Pathway

A

The specific conditions that determine how energy transfer is divided between work and heat

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8
Q

State function (property)

A

A property that is independent of the pathway

e.g.: Energy change, internal energy, pressure, volume, enthalpy

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9
Q

System

A

Part of the universe on which we wish to focus attention

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10
Q

Surroundings

A

Everything else in the universe

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11
Q

Exothermic

A

Energy flows out of the system

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12
Q

Endothermic

A

Energy flows into the system

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13
Q

Thermodynamics

A

The study of energy and its interconversions

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14
Q

The First Law of Thermodynamics

A

The energy of the universe is constant

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15
Q

Internal energy

A

The sum of the kinetic and potential energies of all the “particles” in the system

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16
Q

Change in internal energy

A 
∆E = q + w
E = internal energy
q = heat
w = work
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17
Q

When q is positive…

A

A quantity of energy flows into the system via heat (an endothermic process)

18
Q

When q is negative…

A

A quantity of energy flows out of the system via heat (an exothermic process)

19
Q

When w is positive…

A

The surroundings do work on the system (energy flows into the system)

20
Q

When w is negative…

A

The system does work on the surroundings (energy flows out of the system)

21
Q

Work equation

A

Compression: Work = P x A x ∆h = P∆V
Expansion: Work = -P∆V

22
Q

Enthalpy

A 
H = E + PV
H = enthalpy
E = internal energy of the system
P = pressure of the system
V = volume of the system
23
Q

At constant pressure (where only PV work is allowed)…

A

The change in enthalpy ∆H of the system is equal to the energy flow as heat q (Heat of reaction = change in enthalpy)

24
Q

Enthalpy change equation

A

∆H = Hproducts - Hreactants

25
Q

When ∆H is positive…

A

The products of a reaction have a greater enthalpy than the reactants, so heat will be absorbed by the system (ENDOTHERMIC)

26
Q

When ∆H is negative…

A

The reactants of a reaction have a greater enthalpy than the products, so heat will be generated by the system (EXOTHERMIC)

27
Q

Calorimeter

A

The device used experimentally to determine the heat associated with a chemical reaction

28
Q

Calorimetry

A

The science of measuring heat based on observing the temperature change when a body absorbs or discharges energy as heat

29
Q

Heat capacity

A

C = heat absorbed / increase in temperature

30
Q

Specific heat capacity

A

The energy required to raise the temperature of one gram of a substance by one degree Celsius

31
Q

Molar heat capacity

A

The energy required to raise the temperature of one mole of a substance by one degree Celsius

32
Q

Energy (as heat) equation

A 
q = s x m x ∆T
s = specific heat capacity
m = mass of solution
∆T = increase in temperature
33
Q

Constant volume calorimetry equation

A 
q = s x ∆T  
s = specific heat capacity of the calorimeter
34
Q

Hess’s Law

A

In going from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps

35
Q

Standard enthalpy of formation (∆H˚f)

A

The change in enthalpy that accompanies the formation of 1 mole of a compound from its elements with all substances in their standard states

36
Q

Law of Summation of Heats of Formation

A

∆H˚reaction = sum of the heats of formation for the products multiplied by their coefficients in a balanced chemical equation - sum of the heats of formation for the reactants multiplied by their coefficients in a balanced chemical equation

37
Q

Fossil fuels

A

Coal, petroleum, or natrual gas

38
Q

Petroleum

A

A thick, dark liquid composed mostly of compounds called hydrocarbons that contain carbon and hydrogen

39
Q

Natural gas

A

Usually associated with petroleum deposits, consists mostly of methane, but it also contains significant amounts of ethane, propane, and butane

40
Q

Coal

A

Formed from the remains of plants that were buried and subjected to high pressure and heat over long periods of time

41
Q

Greenhouse effect

A

A warming effect exerted by the earth’s atmosphere (particularly CO2 and H2O) due to thermal energy retained by absorption of infrared radiation

42
Q

Syngas

A

Synthetic gas, a mixture of carbon monoxide and hydrogen, obtained by coal gasification

AP Chemistry (10 decks)

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