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gen chem > ch 7 > Flashcards

ch 7 Flashcards

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1
Q

energy

A

capacity to do work

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2
Q

work

A

force acting through a distance

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3
Q

heat

A

flow of energy caused by a temp difference

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4
Q

kinetic energy

A

energy associated with motion

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5
Q

thermal energy

A

type of KE associated with the temperature

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6
Q

potential energy

A

energy associated with the position or composition of an object

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7
Q

chemical energy

A

type of PE associated with the positions of electrons/nuclei in atoms and molecules

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8
Q

law of conservation of energy

A

energy cannot be crated or destroyed

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9
Q

KE formula

A

KE= 1/2mv^2

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10
Q

SI unit of energy

A

Joule (J) = kg x m^2/s^2

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10
Q

SI unit of energy

A

Joule (J) = kg x m^2/s^2

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11
Q

SI unit of energy

A

Joule (J) = kg x m^2/s^2

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11
Q

SI unit of energy

A

Joule (J) = kg x m^2/s^2

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12
Q

specific heat

A

amount of energy required to raise the temp of 1 g of water by 1 degree C

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13
Q

1 cal = _____ J

A

4.184 J

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14
Q

Calorie (Cal)=

A

1 Cal = 1kcal = 1000 cal

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15
Q

thermodynamics

A

study of energy and its interconversions

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16
Q

first law of thermodynamics

A

total energy of the universe is constant

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17
Q

Internal Energy (E)

A

sum of the Ke and PE of all particles that compose the system

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18
Q

internal energy is a ____ function.

A

state function: its value depends only on the state of the system, not how it arrived at that state.

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19
Q

ΔE=

A

ΔE= E(final)-E(initial)

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20
Q

in a chemical system ΔE=

A

ΔE= E(products) - E(reactants)

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21
Q

the amount of energy lost by the system must exactly equal

A

the amount gained by the surroundings

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22
Q

ΔE(system)= -ΔE____

A

-ΔE surroundings

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23
Q

If the reactants have a higher internal energy than the products, ΔE…

A

is negative and energy flows out of system into surroundings

24
Q

If the reactants have a lower internal energy than the products, ΔE…

A

is positive and energy flows into system from surroundings

25
Q

thermal energy flows from

A

flows from matter at higher temperatures to matter at lower temperatures

26
Q

thermal equilibrium

A

point at which there is no additional net transfer of heat between a system and its surroundings

27
Q

heat capacity (C)

A

a measure of the system’s ability to absorb thermal energy without undergoing a large change in temp

28
Q

the higher the heat capacity of a system

A

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

29
Q

heat capacity is defined as

A

the quantity of heat required to change its temp by 1 degree C

30
Q

heat capacity is an extensive property , why?

A

it depends on the amount of substance being heated

31
Q

specific heat capacity (Cs)

A

amount of heat required to raise the temp of 1g of the substance by 1 degree C

32
Q

molar heat capacity

A

amount of heat required to raise the temp of 1 mole of substance by 1 degree C

33
Q

specific heat capacity and molar heat capacity are ___ properties

A

intensive (depends on the KIND of substance)

34
Q

water has a very ____ specific heat capacity

A

high

35
Q

pressure-volume work

A

work that occurs when a volume change takes place against an external pressure

36
Q

heat at constant volume (qv) is equal to

A

ΔErxn

37
Q

in colorimetry we…

A

measure the thermal energy exchanged between the reaction and the surroundings by observing the change in temp of the surroundings

38
Q

bomb calorimeter

A

piece of equipment that measures ΔE for combustion reactions

39
Q

enthalpy (H)

A

the sum of a systems internal energy and the product of its pressure and volume

40
Q

ΔE is a measure of ______ while ΔH is a measure of only ________

A

all of the energy; only the heat exchanged under constant pressure

41
Q

endothermic reaction

A

ΔH is positive; absorbs heat from its surroundings

42
Q

example of endothermic reaction

A

cold pack

43
Q

exothermic reaction

A

ΔH is negative; gives off heat to its surroundings

44
Q

breaking bonds always _____ energy.

A

absorbs

45
Q

in an endothermic reaction, _____ bonds break and ____ bonds form.

A

weak, strong; resulting in net energy production

46
Q

heat of reaction (ΔHrxn)

A

enthalpy change for a chem reaction; depends on the amount of material undergoing the reaction

47
Q

coffee cup calorimetry occurs at constant ___ and measures ___ for a reaction

A

pressure; ΔH

48
Q

bomb calorimetry occurs at constant ___ and measures ____ for a reaction.

A

volume; ΔE

49
Q

standard state for a gas

A

the pure gas at a pressure of exactly 1 atm

50
Q

standard state for liquid or solid

A

the pure substance in its most stable form at 1 atm and the temperature of interest

51
Q

standard state for a substance in solution

A

a concentration of exactly 1 M

52
Q

standard enthalpy change (ΔH°)

A

the change in enthalpy for a process when all reactants and products are in their standard states (degree sign indicates standard states)

53
Q

standard enthalpy of formation ΔH°f for a pure compound

A

the change in enthalpy when 1 mol of the compound forms from its constituent elements in their standard states

54
Q

standard enthalpy of formation ΔH°f for a pure element it its standard state

A

ΔH°f= 0

55
Q

negative standard enthalpy of formation ΔH°f

A

decomposition of a compound into its constituent elements

56
Q

sulfur oxides are ___ and ___ irritants that affect…

A

lung, eye; the respiratory system and are the main precursors of acid rain

57
Q

carbon monoxide displaces ____ in the blood, causing…

A

oxygen; the heart and lungs to work harder

58
Q

ground level ozone is a…

A

lung/eye irritant; prolonged exposure can cause lung damage

59
Q

CO2 is a greenhouse gas, so it

A

allows visible light form the sun to enter our atmosphere, but prevents heat from escaping

gen chem (12 decks)

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