thermochemistry Flashcards

1
Q

theres two kinds of basic energy:

A

Potential (stored) and kinetic (motion)

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2
Q

Internal energy =

A

sum of all energy

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3
Q

On molecular scale, chemical bond energy =

A

potential energy stored in molecular clouds

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4
Q

energies of molecular moition =

A

Rotationa;, translational, vibrational

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5
Q

thermal energy

A

sometimes called energy of molecular motion

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5
Q

temperature is a common measure of

A

energy of molecular motion

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6
Q

ENERGY is the capacity to

A

do work or supply heat

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7
Q

1st law of thermodynamics

A

energy cannot be created or destroyed

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8
Q

All total energy of universe is ____

A

conserved

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9
Q

UNiverse equation

A

system + surroundings

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10
Q

If energy leaves the system, it must

A

enter the surroudings

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11
Q

energy change in energy system has to be accompanied by an _______ _______ change and the ____ must be ________

A

equal magnitude

signs

opposite

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12
Q

ΔE =

A

Eproducts - E reactants

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13
Q

state function

A

A function or property whose value depends only on the present state (condition) of the system (path doesn’t matter)

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14
Q

Example of state function

A

Arriving to Montreal with or with out layovers doesn’t matter. final position is the state function

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15
Q

Most changes to internal energy of system involve ______ of both _____ & ______

A

transfer

heat

work

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16
Q

ΔESYS =

A

work (w) - heat (q)

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17
Q

If w (work) = 0 then

A

it is example of energy transferred only as heat (q)

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18
Q

Heat or thermal energy will flow from _________ to _________ objects, eventually reaching _________ __________

A

higher-temp

lowe-temp

equal temp

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19
Q

When w = 0, ΔE < 0, q < 0 then

A

heat released to surrounding
(E initial > E final)

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20
Q

When w = 0, ΔE > 0, q > 0 then

A

heat absorbed to surrounding
(E intial < E final)

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21
Q

Mechanical work is the product of

A

w = force (F) x distance (d)

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22
Q

The larger the force or the longer the distance an object is moved, ….

A

the more work is done ON it

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23
Q

when is transfer of energy work only

A

when q = 0

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24
When gas forming rxn in insulated container is attached to piston cylinder that pushes against it, the system
pushes the piston out, DOING WORK ON the surroundings
25
Expansion work
The work done when the volume of a system changes in the presence of an external pressure
26
Expansion work i also known as
Pressure volume work
27
Expansion work at constant pressure (P = P surroundings) the formula is
w = -PΔV = -P(V final - Vinitial)
28
More work is done when the volume change is
larger
29
The sign of expansion work is negative because
The system is expanding and doing work. It LOSES internal energy by doing this work
30
If the volume occupied by the reactants is larger than the volume occupied by the products,
Work is done on the system
31
Enthalpy is a scale to keep track of the ______ of the _______________ transformation
energenetics constant-pressure
32
ENTHALPY (H) is defined as
H = E + PV
33
Change in enthalpy (ΔH) formula
ΔH = ΔE +PΔV
34
Change in enthalpy (ΔH) is equal to the amount of heat ________ or ______ in a ________ at CONSTANT PRESSURE
gained loss transformation
35
if ΔH < 0 then if ΔH > 0 then
exothermic (heat loss, is a product) endothermic (heat gain, is a reactant)
36
Multiplying a reaction increases ΔH by reversing a reaction changes
by the same factor the sign of ΔH
37
heat capacity definition
amount of heat required to raise the temperature of an object or substance by 1C or K
38
Heat capacity formula
q/ΔT
39
Sand heats up really quick so it has _____ heat capacity
LOW
40
Specific heat capacity definition and formula
Heat capacity per mass (1g) c = q/(mass x ΔT)
41
Molar heat capacity definition and formula
Heat capacity per mole c = q/ (amount mole x ΔT)
42
Energy is stored in different _______________
degrees of motion
43
Higher heat capacity means _____ ________ given off
more heat
44
Calorimetry
Science of measuring the heat exchanged in chemical reactions
45
In calorimetry, the heat of reaction (qrxn) is measured __________ by means of a calorimeter. If rxn produces heat, the temperature of surroundings _________ and vice versa
indirectly increases
46
q rxn =
- q calorimeter = -(qvessel + qsolution +qother)
47
example of constant pressure or coffee cup calorimetry
qsys (sample) = -q calorimeter (surrounding h20)
48
HEAT CAPACITY of the calorimeter (often equal ot that of the surrounding water cuz heat absorption of vessel is minimal) provides the link between _____________ and _________ from which you can determine the _____ ______ of the system
ΔT Heat gained/lost enthalpy change
49
Heat capacity (calorimeter) formula
q cal/ΔT cal
50
Standard states of pure substance gas substance in aquoeous solution
1atm 1 atm 1M concentration
51
Standard enthalpy of a reactioon is indicated by symbol
ΔH° rxn
52
what does ΔH° rxn indicate`
enthalpy change noted corresponds to all reactants and all products being present IN Standard state
53
symbol for standard enthalpies of formation also called standard heat of formation
ΔH°f
54
ΔH°f is enthalpy change for the formation of ________ of substance in its ________ from its ________ elements in their standard states
1 mole standard state constituent
55
ΔH°f FORMULA
ΔH°f = ΔH°f (PRODUCTS) - ΔH°f (REACTANTS)
56
ΔH°f CAN BE approximated by
accounting for bonds broken and formed using fomrula ΔHrxn° ~~ BE (reactant bonds) - BE (product bonds)
57
Hess law is
ΔH overall = ΔH1 + ΔH2 + ΔH3 .......
58
what is texts notation for hess hlaw:
it uses ∑mΔH°f(products) - ∑nΔH°f(reactants)
59
∑ is m and n
sum of all m and n is stoichiometric coefficients
60
Explain work done ON vs work done BY
Work done on = something outside increases the energy inside the system work done by = systems internal energy decreased when it did work. (DONE BY* SYSTEM DOES THE WORK)