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Chemistry 1 > Chapter 7 > Flashcards

Chapter 7 Flashcards

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1
Q

is the study of the
relationship between energy and matter.

A

Thermochemistry

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2
Q

is anything that has the capacity to
do work.

A

energy

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3
Q

is a force acting over a distance

A

work

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4
Q

is the flow of energy caused by a difference in temperature between objects.

A

Heat

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5
Q

is energy of motion or
energy that is being
transferred.

A

Kinetic energy

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6
Q

is the energy associated with temperature.

A

thermal energy

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7
Q

is energy that is stored in an object (e.g. bond energy), or energy associated with the position of the object.

A

Potential energy

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8
Q

Energy stored in the structure of a compound is

A

chemical
potential energy.

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9
Q

associated with positions of electrons and nuclei

A

chemical energy

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10
Q

Kinetic energy associated with the flow of electrical charge

A

electrical energy

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11
Q

Kinetic energy associated with energy transitions in an atom

A

Light or radiant energy

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12
Q

Potential energy in the nucleus of atoms

A

nuclear energy

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13
Q

Potential energy due to the structure of the atoms, the
attachment between atoms, the atoms’positions relative to
each other in the molecule, or the molecules’ relative
positions in the structure

A

chemical

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14
Q

states that energy
cannot be created nor
destroyed.

A

law of conservation of
energy

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15
Q

as the material or process within which
we are studying the energy changes within.

A

system

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16
Q

as everything else with which the system can exchange energy.

A

surroundings

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17
Q

is the study of the exchange of energy
between the system and the
surroundings.

A

thermochemistry

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18
Q

that the amount of
energy gained or lost by the system has to be equal to the amount of energy lost or gained by the surroundings.

A

conservation of energy

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19
Q

is the amount of energy needed to
move a 1 kg mass a distance of 1 meter.

A

joule (J)

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20
Q

is the amount of energy needed to
raise the temperature of one gram of water 1 o C.

A

calorie (cal)

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21
Q

is the study of energy and its
interconversions.

A

thermodynamics

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22
Q

conversion for calorie to joules

A

1 calorie = 4.184 joules

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23
Q

what is the other name for the law of conservation of energy

A

The First Law of Thermodynamics

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24
Q

of a system is the sum of the kinetic and potential energies of all of the particles that compose the system.

A

internal energy (E)

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25
Q

is a mathematical function whose result only
depends on the initial and final conditions, not on the process used.

A

state function

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26
Q

the height from the base to the peak of the
mountain is a state function

A

altitude

27
Q

When energy flows out of a
system, E system is

A

negative

28
Q

When energy flows into the
surroundings, E surroundings is

A

positive

29
Q

Heat exchange at constant pressure is
called the

A

enthalpy

30
Q

are a “graphical”way of showing the direction of energy flow during a process.

A

Energy diagrams

31
Q

Energy is exchanged between the system and
surroundings through

A

heat and work

32
Q

symbol for heat energy

A

q

33
Q

symbol for work energy

A

w

34
Q

is the heat capacity.

A

C

35
Q

what does the heat of capacity of an object depend on

A

the mass and the type of material

36
Q

is the amount of heat energy required to raise
the temperature of one gram of a
substance 1 degree C.

A

specific heat capacity

37
Q

is the amount of heat energy required to raise the
temperature of one mole of a
substance 1 degree C.

A

molar heat capacity

38
Q

what is work caused by?

A

a change in volume against an external
pressure

39
Q

a chemical reaction occurs open
to the atmosphere under conditions of what?

A

constant pressure

40
Q

Heat exchange at constant pressure is
called the

A

enthalpy

41
Q

device used to measure enthalpy

A

the coffee-cup caloriemeter

42
Q

of a system is defined as the sum of the
internal energy of the system (E) and the product of pressure (P) and volume (V):

A

enthalpy (h)

43
Q

what is the symbol for enthalpy

A

H

44
Q

Hand Ehave the largest difference for reactions that produce or use what

A

large quantities of gas.

45
Q

the products of the reaction have less
chemical potential energy than the reactants.

A

exothermic reaction,

46
Q

what does a negative delta h mean?

A

exothermic reaction

47
Q

what does a positive delta h mean?

A

endothermic reaction

48
Q

where does the extra thermal energy come from?

A

the conversion of
some of the chemical potential energy in the reactants
into kinetic energy in the form of heat.

49
Q

The enthalpy change in a chemical reaction is an

A

extensive property

50
Q

The surrounding area is called a

A

bomb calorimeter

51
Q

device used to measure delta E

A

the bomb calorimeter

52
Q

why is the the bomb calorimeter used?

A

bc it has a constant volume system

53
Q

is the amount of
heat absorbed by the
calorimeter for each degree
rise in temperature

A

the heat capacity of the calorimeter

54
Q

heat capacity of the
calorimeter

A

calorimeter constant.

55
Q

As something rolls on the table, some of the energy is converted to heat by

A

friction

56
Q

is the exchange of thermal energy between a system
and surroundings.

A

heat

57
Q

Heat exchange occurs when system and surroundings
have a what?

A

difference in temperature.

58
Q

is the measure of the thermal energy within a sample of matter.

A

temperature

59
Q

Heat flows from matter with high temperature to matter with low temperature until both objects reach the same
temperature.

A

Thermal equilibrium

60
Q

heat flows from the material at the ?
temperature to the material at the ? temperature.

A

higher to lower

61
Q

Heat flows until both materials reach the same final
temperature –

A

Thermal Equilibrium

62
Q

The amount of heat energy lost by the hot material
equals what?

A

the amount of heat gained by the cold material.

63
Q

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

A

Hess’s Law

64
Q

is the enthalpy
change when all reactants and products are in their standard
states.

A

standard enthalpy change for a reaction

Chemistry 1 (14 decks)

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