Module 13 Flashcards

1
Q

Hess’s Law

A

Enthalpy is a state function and is therefore independent of path.

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2
Q

State function

A

any quantity that depends solely on the final destination, not on the way you get to that destination

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3
Q

for enthalpy, the amount of energy contained in a substance is

A

independent of how it is made

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4
Q

enthalpy of formation (ΔHf)

A

the ΔH of a formation reaction

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5
Q

standard conditions

A

a temp of 25 C and a pressure of 1.00 atm

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6
Q

standard enthalpies of formation

A

the ΔHf for molecules under standard conditions

denoted with an “°”

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7
Q

the ΔH° of any chemical reaction is the

A

sum of the ΔHf° for the products minus the sum of the ΔHf° for the reactants

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8
Q

when a reaction is exothermic energy will be thought of a s

A

a product in the reaction

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9
Q

when a reaction is endothermic energy will be thought of as

A

a reactant in the reaction

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10
Q

enthalpy

A

the energy stored in a substance
stated as the ‘enthalpy of that substance’
symbolized by ‘H’

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11
Q

change in enthalpy (ΔH)

A

the energy change that accompanies a chemical reaction

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12
Q

1 calorie =

A

4.184 Joules

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13
Q

ΔH is positive for – reactions and negative for – reactions

A

endothermic

exothermic

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14
Q

whether a reaction is exothermic or endothermic, energy is both– and– during the course of the reaction. the difference is —

A

absorbed
released
how much

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15
Q

bond energy

A

the strength of a chemical bond

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16
Q

ΔH=

A

energy required to bread bonds/ energy released when bonds form

17
Q

the standard enthalpy of formation of an element in its elemental form is

A

zero

18
Q

energy diagram

A

a ‘picture’ of the energy associated with a chemical reaction

19
Q

reaction coordinate

A

tells us how close the reaction is to completion

plotted on the horizontal/ x axis of the graph

20
Q

intermediate state/ activated complex

A

occurs at the top of the hump, which represents the midpoint of the reaction

21
Q

activation energy

A

the energy necessary to start a chemical reaction

22
Q

entropy

A

a measure of the disorder that exists in any system

denoted by an ‘S’

23
Q

2nd law of thermodynamics

A

the entropy of the universe must always either increase or remain the same. It can never decrease

24
Q

which state has the least amount of entropy associated with it? How about the middle amount? What about the highest amount?

A

solid
liquid
gaseous

25
Q

the entropy of a system increases with – temp

A

increasing

26
Q

the entropy of a system increases os the matter it contains–

A

increases

27
Q

ΔS universe ≥

A

0

28
Q

all substances, even elements have

A

an absolute entropy

29
Q

what does the Gibbs Free equation tell us?

A

whether or not a reaction is consistent with the second Law of thermodynamics

30
Q

if a reaction is consistent with the second law, we call it

A

spontaneous

this is because we know that it con proceed

31
Q

if a reaction is ‘not spontaneous’ it means;

A

The reaction is not consistent with the second law and therefore cannot occur

32
Q

when ΔG

A

is consistent with the second law

is spontaneous

33
Q

when ΔG > 0 the reaction

A

is not consistent with the second law
cannot proceed
is not spontaneous