Chapter 8 Flashcards

1
Q

Thermodynamics

-thermochemistry

A

The study of energy and temperature changes

- energy changes in chemical reactions

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2
Q

Energy is:

A

the ability to do work

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3
Q

Forms of energy:

  • Potential energy:
  • Kinetic energy
A
  • stored energy

- energy of motion

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4
Q

Types of energy changes:

  • Heat:
  • Work:
A
  • the transfer of kinetic energy

- the transfer of energy from one form to another

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5
Q

1000 calories=

A

1 kcal = 1 Calorie

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6
Q

1 calorie (c) =

A

4.184 J

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7
Q

Change in energy:

A

ΔE = q+w (Total energy released = sum of heat (q) and work (w)

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8
Q

Exothermic change

A
releases energy (sometimes depicted as +energy on the R side of a chemical equation)
releases heat energy: -q
system does work on surroundings: -w
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9
Q

Endothermic change

A
Absorbs change (sometimes depicted as +energy on the L side of a chemical equation)
absorbs heat energy: +q
surroundings does work on system: +w
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10
Q

In thermochemistry:

  • The System:
  • the surroundings:
A
  • is the part of the universe being studied

- the rest of the universe

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11
Q

The law of conservation of energy

A

Energy cannot be created or destroyed

ΔE system = -ΔE surroundings

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12
Q

Heat energy and temperature

A

Heat: the t o t a l kinetic energy transferred from one object to another
Temperature: the a v e r a g e kinetic energy of the particles in a substance

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13
Q

Specific heat

A

the relationship between heat mass and temp

the amount of heat required to raise the temperature of one gram of material by 1*C

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14
Q

Equation for specific heat

A

specific heat = (heat)/ ((mass)x(change in temperature))
s=q/mΔT
q=msΔT

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15
Q

Heat capacity, C

A

the amount of heat required to raise a substance by 1*C

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16
Q

Heat capacity equation

A

heat capacity = q/ΔT

C= q/ΔT

17
Q

Calorimetry experiments

A

measure the flow of heat

18
Q

coffee cup calorimetry

A

q water = -q metal
(w and 2nd m’s are subscripts)
mwswΔTw=-mmsmΔTm

19
Q

fuel value

A

the amount of energy that can be produced by the combustion of a material
the higher the fuel value the more energy it releases when it burns

20
Q

reaction enthalpy

A

the amount of heat energy absorbed or released in a chemical reaction at a constant pressure
ΔHrxn
allows us to relate the heat changes in a reaction to the amount of any substance involved in the reaction.