Chapter 7 Flashcards

1
Q

Thermochemistry

A

study of the relationships between chemistry and energy

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2
Q

Energy

A

capacity to work

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3
Q

Work

A

the result of a force acting through a distance

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4
Q

heat

A

the flow of energy by a temperature difference

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5
Q

kinetic energy

A

energy associated with the motion of an object

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6
Q

Thermal energy

A

energy associated with the temperature of an object

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7
Q

potential energy

A

energy associated with the position or composition of an object

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8
Q

chemical energy

A

energy is associated with the relative positions of electrons and nuclei in atoms and molecules

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9
Q

law of conservation of energy

A

energy can be neither created nor destroyed

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10
Q

surrounding

A

everything with which the system can exchange energy

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11
Q

kinetic energy

A

1/2 mv^2
m- kg
v- m/s
kinetic energy - J

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12
Q

1 calories (cal) to Joules (J)

A

1 cal = 4.184 J

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13
Q

kilo watt per hour to joules

A

1 kWh = 3.60 x 10^6 J

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14
Q

thermodynamics

A

the general study of energy and its interconversions

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15
Q

first law of thermodynamics

A

the total energy of the universe is constant

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16
Q

internal energy (E)

A

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

17
Q

The internal energy of a chemical system

A

delta E = E(products) - E(reactants)

18
Q

Reactants have a higher internal energy than the products

A

delta E(sys) Is negative
-energy flows out of the system into the surroundings

19
Q

reactants have a lower internal energy than the products

A

delta E(sys) is postive
energy flows into the system from the surroundings

20
Q

Change in thermal energy of the system

A

heat transfer (q) + work done (w)

21
Q

when q is positive

A

system gains thermal energy

22
Q

when q is negative

A

system loses thermal energy

23
Q

when w is positive

A

work down on the system

24
Q

when w is negative

A

work done by the system

25
Q

when a change in internal energy is positive

A

energy flows into the system

26
Q

when a change in internal energy is negative

A

energy flows out of the system

27
Q

Delta E(sys)

A
  • delta E (surr)
28
Q

higher the heat capacity of a system

A

smaller the change in temperature for a given amount of absorbed heat

29
Q

The formula for F, W, D

A

Work = work as a force (F) x acting through a distance (D)

30
Q

the formula for F, P, A

A

Force = external pressure (P ext) x Area the pressure acts on (A)

31
Q

The formula for W, P, V

A

Work = -Pext x change in volume

32
Q

Enthalpy (H)

A

a system as the sum of its internal energy and the product of its pressure and volume

33
Q

Formula for enthalpy

A

H = change in E + P (change in V)

34
Q

Endothermic reaction

A

chemical reaction with a positive H
- absorbs heat from its surroundings
- strong bonds break to form weak bonds

35
Q

Exothermic reaction

A

chemcial reaction with a negative H
- weak bonds break to form strong bonds

36
Q

standard delta H(rxn)

A

sum of (delta Hf products x stoichiometry) - sum of (delta Hf reactants x stoichiometry)