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AP Chemistry > Chapter 6 Quiz > Flashcards

Chapter 6 Quiz Flashcards

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1
Q

Thermochemistry

A

The study of the relationship between chemistry & energy

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2
Q

Work

A

The result of a force acting through a distance

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3
Q

Heat

A

The flow of energy caused by temp. difference

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4
Q

Kinetic energy

A

The energy associated with the motion of an object

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5
Q

Thermal energy

A

The energy associated with the temperature of an object

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6
Q

Potential energy

A

The energy associated with the position or composition of an object

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7
Q

Chemical energy

A

The energy associated with the relative positions of electrons & nuclei in atoms & molecules (form of potential energy)

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8
Q

Law of conservation of energy

A

States that energy can neither be created nor destroyed

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9
Q

System

A

A set of substances & energy that are being studied

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10
Q

Surroundings

A

Everything with which the system can exchange energy

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11
Q

KE =

A

1/2mv^2
1/2(mass)(velocity^2)

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12
Q

1kg m^2/s^2

A

1 joule (J)

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13
Q

calorie (cal)

A

4.184 J

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14
Q

Calorie (Cal)

A

4184 J

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15
Q

Joules

A

SI unit of energy

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16
Q

First law of thermodynamics

A

The total energy of the universe is constant / does not change

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17
Q

Internal energy

A

The sum of kinetic & potential energies of all of the particles that compose the system. It is a state function

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18
Q

State function

A

The value depends only on the state of the system

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19
Q

ΔE =

A

E(final) - E(initial)
E(products) - E(reactants)
q + w OR heat + work

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20
Q

When is ΔE positive?

A

When energy is absorbed (endothermic reaction)

21
Q

When is ΔE negative?

A

When energy is released

22
Q

Thermal equilibrium

A

There is no additional net transfer of heat

23
Q

Heat capacity (C)

A

A measure of the system’s ability to absorb thermal energy without undergoing a large change in temp OR the amount of heat required to change its temperature by 1 degree C.

24
Q

Specific heat capacity (Cs)

A

The amount of heat required to raise the temp of 1 gram of substance by 1 degree C

25
Q

Molar heat capacity

A

The amount of heat required to raise the temp of 1 mol of a substance by 1 degree C

26
Q

q =

A

m times Cs times ΔT
Heat (J) = mass (g) times Specific heat capacity (J/gC) times Temp change (degrees C)

27
Q

Pressure-volume work

A

Occurs when force is caused by a volume change against an external pressure

28
Q

w =

A

f times d OR force times distance
p times a times d
p times a times Δh
p times ΔV

29
Q

ΔE(rxn) =

A

qv+w

30
Q

Calorimetry

A

measuring the thermal energy exchanged between the reaction (or system) and the surroundings by observing the change in temp of the surroundings

31
Q

Bomb calorimeter

A

Piece of equipment designed to measure ΔE for combustion reactions

32
Q

q(cal) =

A

C(cal) times ΔT
C(cal) = heat capacity of the entire calorimeter assembly

33
Q

Enthalpy

A

The sum of a system’s internal energy & the product of its pressure & volume

34
Q

ΔH =

A

ΔE + PΔV
the heat at constant pressure

35
Q

Endothermic reaction

A

A chemical reaction that absorbs heat from its surroundings

36
Q

Exothermic reaction

A

A chemical reaction that releases heat to its surroundings

37
Q

When is ΔH positive?

A

When it’s endothermic

38
Q

When is ΔH negative?

A

When it’s exothermic

39
Q

Enthalpy of reaction / Heat of reaction

A

Extensive property - depends on the amount of material undergoing the reaction. The enthalpy change for a chemical reaction

40
Q

Coffee-cup calorimeter

A

Consists of 2 styrofoam coffee cups, one inserted into the other, to provide insulation from the laboratory equipment. Equipped with a thermometer & stirrer

41
Q

Compare & contrast bomb calorimeters & coffee-cup calorimeters

A

Bomb calorimeters & coffee-cup calorimeters both measure changes in temp. However, bomb calorimeters measure ΔE & have constant volume while coffee-cup calorimeters measure ΔH(rxn) & have constant pressure

42
Q

Relationships involving ΔH(rxn)

A
  1. If a chemical equation is multiplied by the same factor, then ΔH(rxn) is also multiplied by the same factor
  2. If a chemical equation is reversed, then ΔH(rxn) changes signs
  3. If a chemical equation can be expressed as the sum of a series of steps, then ΔH(rxn) for the overall equation is the sum of the heats of reactions for each step
43
Q

Hess’s Law

A

The change in enthalpy for a stepwise process is the sum of the enthalpy changes of the steps

44
Q

Standard state

A

Pure gas at a pressure of exactly 1atm
Pure liquid or solid in its most stable form at a pressure of 1atm & at the temp of interest (usually 25 degrees C)
Substance in solution at a concentration of exactly 1M

45
Q

Standard enthalpy change (ΔH w/ degree sign)

A

The change in enthalpy for a process when all reactants & products are in their standard states. The degree sign indicates standard states

46
Q

Standard enthalpy (heat) of formation (ΔH(f) w/degree sign)

A

ΔH(f) w/ degree sign = 0 for a pure element in its pure state.
For a pure compound: The change in enthalpy when 1 mol of the compound forms its constituent elements in their standard states

47
Q

ΔH (w/ degree sign) (rxn)

A

Sum of n(p) times ΔH (w/ degree sign) (products) - Sum of n(r) times ΔH (w/ degree sign) (reactants)

48
Q

List 3 connections between energy use & the environment

A
  • Ozone production
  • CO2
  • Solar panels
49
Q
A

AP Chemistry (1 decks)

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