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Introduction to Chemistry > chapter 7: chemical energy > Flashcards

chapter 7: chemical energy Flashcards

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1
Q

what is thermodynamics

A

the study of energy and its transformations

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2
Q

what is thermochemistry

A

relationship between chemical reactions and energy changes involving heat

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3
Q

what is energy

A 
the ability (or capacity) to do work or 
transfer heat.
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4
Q

what is work

A

Energy used to cause
an object that has mass
to move

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5
Q

what is heat

A

Energy used to cause
the temp of an object
to rise

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6
Q

what is force

A

any kind of push or pull exerted on an object

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7
Q

what is the formula for force

A

f = m x g

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8
Q

what does g stand for

A

acceleration due to gravity; 9.8 m/s^2

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9
Q

what is the magnitude of work formula

A 
w = F x d = m x g x d
d = distance
m = mass
F = force
g = gravity
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10
Q

what is another name for heat

A

thermal energy

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11
Q

what direction does heat flow

A

warmer objects to cooler objects

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12
Q

what are some characteristcs of heat and work

A
  • energy is being exchanged between two objects
  • energy can flow into or out of the subject studied
  • dont exist before or after the state of change
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13
Q

what types of energy are there

A

potential and kinetic

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14
Q

what is electrical energy

A

KE associated w/ flow of electrical charge

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15
Q

what is heat or thermal enrgy

A

KE associated w/ molecular motion

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16
Q

what is light or radiant energy

A

KE associated with energy transitions in an atom

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17
Q

what is nuclear energy

A

PE in the nucleus of atoms

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18
Q

what is chemical energy

A

PE due to the structure of the atoms

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19
Q

what is kinetic energy

A

energy that is being transferred (motion)

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20
Q

what is the kinetic energy formula

A

KE = 1/2mv^2

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21
Q

what does KE depend on

A

the mass and speed of the object

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22
Q

do atoms and molecules possess KE

A

yes

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23
Q

what is potential energy

A

energy that is stored in an object

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24
Q

when does PE arise

A

no force operating on the on

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25
what does PE depend on
mass, height, the gravitational
26
what is the formula for PE
m x g x h
27
what is the unit for energy
Joule (J)
28
who was the energy SI unit named after
James Joule
29
what does 1 joule equal
1 kgm^2/ s^2
30
what is a non-SI unit that is still used
calorie (cal)
31
how many joules does one calorie equal
4.184 J
32
what is the value of the nutritional calorie
1000 cal (1kcal)
33
what is the system
included the molecules we want to study
34
what are the surroundings
everything else
35
what is temperature
measure of the kinetic energy, | thermal energy, within a sample of mater.
36
what is thermal equilibrium
the flow of heat from high temp to low temp until both objects reach the same temp
37
what does endothermic mean
heat is absorbed by the system from the surroundings
38
what does exothermic mean
eat is released by the system to | the surroundings,
39
what is the first law of thermodynamics
law of the | conservation of energy.
40
the total energy of the universe it....
constant
41
if the system loses energy...
it must be gained by the surroundings
42
what are state functions
values that depend on the state of the substance, and not on how that state was reached.
43
is delta E a state function
yes bc it depends on the specific amounts of q and w
44
what is an example of a state function
water reached room temp from both directions
45
are q and w state functions
no bc they are forms of energy in transit, don't exist before or after the change of the state
46
what does delta E equal
q + w
47
when does E increase
when heat is added to a system or work is done on a system
48
what does q represent
heat
49
what does w represent
work
50
what happens when q is +
system gains thermal energy
51
what happens when q is -
system loses thermal energy
52
what happens when w is +
work done on the system
53
what happens when w is -
work done BY the system
54
when do most of the chemical and physical changes occur
occur at constant atmospheric pressure
55
what is the formula for pressure-work volume
w = -(P)(change in volume)
56
what is the change in volume
Vfinal - Vinitial
57
when gases expand what happens to the volume and work
``` V = + w = - ```
58
what is enthalpy
heat flow; s defined as the internal energy plus | the product of pressure and volume:
59
what is the formula for enthalpy
H = E +PV
60
what is the formula for enthalpy when system changes at constant pressure, the change in enthalpy,
deltaH = q
61
delta H is positive
endothermic
62
delta H is negative
exothermic
63
what is the formula for enthalpy of a reaction
deltaH = Hproducts - H reactants
64
what is the delta H called
enthalpy of reactionb
65
what are the rules of enthalpy
1.) extensive property
66
what is heat capacity
``` amount of energy required to raise the temp. of a substance by 1 K (1 °C) ```
67
what is specific heat capacity
amount of energy required to raise the temperature of 1 g of a substance by 1 K (1 °C)
68
what is molar heat capacity
the heat capacity of one mole of | a substance is called its
69
what is the formula for heat capacity
Cs = q/ m x deltaT
70
what is the formula for q
m x Cs x change in temp
71
what does Cs mean
specific heat
72
what is calorimetry
measurement of heat flow
73
what is a calorimeter
device used to measure heat flow
74
what happens with the heat produced in a calorimetry reaction
the solution absorbs it
75
what happens to heat in an exothermic reaction
heat is lost by reaction and gained by the solution
76
what happens to heat in an endothermic reaction
heat is gained by the reaction and lost by the solution
77
the heat gained by the solution is equal to...
the magnitude of qrxn
78
what does qsoln =
m x s deltaT = -qrxn
79
what is the constant pressure formula for metal
mass metal x Cs metal x change temp of metal = mass metal x Cs metal x change temp of metal
80
what is the second rule of enthalpy
change of heat for a reaction in the forward direction is equal in magnitude, but opposite in sign, to H for the reverse reaction
81
what is the third rule of enthalpy
H for a reaction depends on the state of the | products and the state of the reactants.

Introduction to Chemistry (12 decks)

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