Chapter 5 Flashcards

1
Q

energy

A

capacity to do work/transfer heat

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2
Q

thermodynamics

A

study of energy and transformations (chemical, mechanical, electrical, etc.)

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3
Q

thermochemistry

A

relationships b/w chemical reactions and energy changes that involve heat
Potential energy- from position

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4
Q

electrostatic potential energy

A

interactions b/w charged particles

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5
Q

E(el) =

A

(kQ1Q2) / d
- Q1/Q2 = electrical charges (2 charge particles)
- d = distance
- k = 8.99 x 10^9 J (m/c^2)
- 1 J = 1 kg m^2/s^2

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6
Q

1st law of thermodynamics

A

energy can be converted from 1 form to another but it is neither created nor destroyed

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7
Q

making bonds

A

releases energy

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8
Q

breaking bonds

A

consumes energy

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9
Q

system

A

portion we single out to study

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10
Q

open system

A

exchange heat and mass w/ surroundings

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11
Q

closed system

A

only exchange heat (not mass) w/ surroundings

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12
Q

isolated system

A

doesn’t exchange heat or mass w/ surroundings

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13
Q

internal energy

A

sum of all kinetic and potential energy of system

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14
Q

∆E =

A

Change in E
∆E = E(final) – E(initial)
∆E = q + w

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15
Q

(+) = E(final) > E(initial)

A

System gained/absorbed energy from surrounding

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16
Q

(-) = E(final)) < E(initial)

A

System lost energy to surrounding

17
Q

q=

A

sum of heat added to/liberated from system
- (+) = system gains heat
- (-) = systems loses heat

18
Q

w=

A

work done on/by system
- (+) = work is done on system
- (-) = work is done by system

19
Q

endothermic

A

system absorbs heat from surroundings
- ∆H = (+)

20
Q

exothermic

A

system releases heat into surrounds
- ∆H = (-)

21
Q

state functions

A

we only care about start & end points; not how we got there

22
Q

work

A

chemical or physical energy –> mechanical work w/ change in volume

23
Q

pressure-volume work; W=

A

W = -P∆V
∆V = V(initial)-V(final)

24
Q

enthalpy (H); ∆H

A

heat at constant pressure
- ∆H = ∆E + P∆V

25
Q

∆H = (+)

A

system gained heat = endothermic

26
Q

∆H = (-)

A

system released heat = exothermic

27
Q

∆H(rxn)=

A

H(products) = H(reactants)

28
Q

calorimetry

A

measurement of heat of flow (∆H)

29
Q

calorimeter

A

device to measure heat flow

30
Q

qsolution =

A

(msolution)( ∆T)(Cs) = -qrxn

31
Q

bomb calorimetry; qrxn =

A

qrxn = Ccal x ∆T
- Ccal = constant (bomb only)

32
Q

heat capacity (C)

A

energy to raise temp of object 1 d K (1 d C)

33
Q

Specific heat capacity Cs=

A

heat capacity of 1 gram of substance
- Cs = q / (m x ∆T)

34
Q

Molar heat capacity (Cm)

A

heat capacity of 1 mole of substance

35
Q

Specific quantity

A

known mass m of substance gains/loses heat

36
Q

Hess’s Law: ∆Hrxn =

A

∆Hrxn = sum of ∆H for each step

37
Q

enthalpies of formation (∆Hf)

A

∆Hf = (n)(∆H)(Hproducts) - (m)(∆H)Hreactants

38
Q

bond enthalpy

A

∆H for breaking of a particular bond in 1 mole of gaseous substance

39
Q

fuel value

A

energy released when 1 g food in combusted