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Chemistry 1 > Chapter 3: Energy and its Conservation > Flashcards

Chapter 3: Energy and its Conservation Flashcards

3.1-3.6

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1
Q

What are the 4 types of energy?

A

Kinetic energy
Potential energy
Thermal energy
Radiant energy

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2
Q

What is kinetic energy?

A

Energy of movement (dependant on the velocity (v) and mass (m) of an object

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3
Q

What is electrical energy?

A

Energy from positive and negative ions held a small distance apart

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4
Q

What is chemical energy?

A

Attraction of the electrons and nuclei in molecules (bond energy)

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5
Q

What is thermal energy?

A

Total energy of random movements of molecules

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6
Q

What is radiant energy?

A

Energy as a result of electromagnetic radiation

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6
Q

What is thermodynamics?

A

The study of energy transfers and transformations

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7
Q

What is the first law of thermodynamics?

A

Energy is neither created nor destroyed, only transferred or transformed from one form into another

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8
Q

What is heat?

A

Thermal energy that is exchanged with its surroundings

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9
Q

What is heat capacity?

A

The quantity of heat required to raise the temperature of the system by 1 degrees celsius or 1 k. Depends on the mass of the heated object

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10
Q

What is molar heat capacity?

A

The amount of heat needed to raise the temperature of 1 mol of substance by 1 degrees celsius

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11
Q

What is specific heat capacity?

A

The amount of heat required to raise the temperature of 1 gram of the substance by 1 degree celsius of 1 k

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12
Q

Do we have to keep track of the signs associated with heat flows? (is energy transfer directional?)

A

Yes. If Tf<Ti, then delta T should be negative

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13
Q

What is work?

A

The energy used to move an object against an opposing force (W surroundings = -W system)

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14
Q

What is a state function?

A

Properties that depend only on the conditions that describe the system (ex. energy)

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15
Q

What are path systems?

A

Depend on how the change occurs (ex. distance; multiple paths to the same spot)

16
Q

Are state and path functions dependant on one another?

A

No.

17
Q

Bond breakage ______ energy

Bond formation ________ energy

A

Requires

Releases

18
Q

What is bond energy? (BE)

A

Energy required to break a bond (always positive)

19
Q

Is the amount of energy released or absorbed in a chemical reaction proportional to the amounts of chemicals that react?

A

Yes (molar ratios)

20
Q

What do bond energies depend on?

A
  1. The types of atoms that are bonded together
  2. The type of bond between two similar atoms
  3. In polyatomic atoms BE depends on the rest of the molecular structure (ex multiple carbons might have different BE even though they are the same element)
21
Q

What does a calorimeter measure?

A

Heat flow from a chemical reaction

22
Q

What is the difference between a constant-pressure calorimeter and a constant-volume calorimeter?

A

Constant-pressure: The volume is changing (used for studying liquids) (styrofoam cup)

Constant-volume: Pressure is changing (used for studying gases) (bomb calorimeter)

23
Q

Does an open system mean constant-pressure, or volume?

Is there work?

What is changing?

A

Constant-pressure

Yes

Volume

24
Q

Does a closed system mean constant-pressure, or volume?

Is there work?

What is changing?

A

Constant-Volume

NO WORK

Pressure

25
Q

What is enthalpy?

A

Describes heat flow at constant pressure

26
Q

Heat flow in a constant-volume process gives:

A

Energy change

27
Q

Heat flow in a constant-pressure process gives:

A

Enthalpy change

28
Q

What is heat of vaporization?

A

Heat required to convert liquid to gas

29
Q

What is heat of sublimation?

A

Heat required to convert solid to gas

30
Q

Formation reactions have what features?

A
  1. A single product with a coefficient of 1
  2. All starting materials are in their standard state
  3. Pressures must be specified
  4. Concentrations must be specified
31
Q

What is a standard state?

A

The most stable form of a substance

at T=25 degrees celsius, p=1 bar, and 1 M if in solution

32
Q

What is the standard molar enthalpy of formation?

A

The standard enthalpy change of a reaction for the formation of 1 mole of a compound directly from its elements

33
Q

What is Hess’s Law?

A

Enthalpy change for any process is equal to the sum of enthalpy changes of the reactants and products since it is independent of the path of the reaction

34
Q

How much of our energy is derived from coal, natural gas, and oil?

A

65%

35
Q

The vast majority of energy sources originate in?

A

Solar energy

Chemistry 1 (6 decks)

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