AP Chem - Chapter 6 - Energy Flashcards

1
Q

what is the law of conservation of energy

A

energy cannot be created nor destroyed

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2
Q

what is energy

A

for our purposes, the capacity to produce heat

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3
Q

what is heat

A

the transfer of energy

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4
Q

what is temperature

A

a measure of kinetic energy

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5
Q

what is the relationship between temperature and kinetic energy

A

directly proportional

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6
Q

what is a state function

A

refers to a property of the system that depends only on its present state. a change in this function in going from one state to another state is independent of the particular pathway taken between the two states

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7
Q

is energy a state function

A

yes

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8
Q

is wrok a state function

A

no

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9
Q

is heat a state function

A

no

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10
Q

what is endothermic

A

refers to a reaction where energy (as heat) flows into the system

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11
Q

what is exothermic

A

refers to a reaction where energy (as heat) flows out of the system

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12
Q

if a reaction has a negative change in H, it is

A

exothermic

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13
Q

if a reaction has a positive change in H, it is

A

endothermic

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14
Q

energy released is

A

exothermic

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15
Q

energy absorbed is

A

endothermic

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16
Q

what is a calorimeter

A

a device used experimentally to determine the heat associated with a reaction

17
Q

what does q stand for

A

heat

18
Q

what is specific heat capacity

A

the amount of energy needed to raise the temp of 1 g of a substance by 1 degree C

19
Q

what are the units for specific heat capacity

A

J/degree C x g

20
Q

is the heat of reaction/change in enthalpy intensive or extensive

A

extensive

21
Q

is temperature intensive or extensive

A

intensive

22
Q

is change in enthalpy a state function

A

yes

23
Q

what is Hess’s law

A

in going from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in one step or a series of steps

24
Q

what happens to the change of H if a reaction is reversed

A

the sign of change of H is reversed

25
Q

what do you do to the value of the change of H if the coefficients in a balanced equation are multiplied by an integer

A

multiply the change of H by the same integer

26
Q

what is standard enthalpy of formation

A

the change in enthalpy that accompanies the formation of one mole of a compound from its elements with all substances in their standard states

27
Q

what are “standard state” temperature and pressure

A

25 degrees celcius

1 atm

28
Q

what is the standard state concentration for a substance in a solution

A

1 M

29
Q

how do you find the change in enthalpy for a given reaction using standard enthalpies of formation

A

using the chart, add the standard enthalpies of formation pf the reactants and of the products (elements are not included; they’re 0). Then multiply each SEF by the amount of moles you have of it. Then subtract what you get for the products from what you got for the reactants.