Term
| When a reaction is exothermic, energy will be thought of as ______________. |
|
Definition
| When a reaction is exothermic, energy will be thought of as a product in the reaction. (417) |
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Term
| When a reaction is exothermic, energy will be considered _______________. |
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Definition
| When a reaction is exothermic, energy will be considered a reactant. (417) |
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Term
| The energy stored in a substance is called the ___________ of that substance. |
|
Definition
|
|
Term
|
Definition
| The energy change that accompanies a chemical reaction. (419) |
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Term
| 1 calorie = ________ Joules |
|
Definition
| 1 calorie = 4.184 Joules (419) |
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Term
ΔH is [positive/negative] for
endothermic reactions. |
|
Definition
|
|
Term
ΔH is [positive/negative] for
exothermic reactions. |
|
Definition
|
|
Term
|
Definition
The energy required
to break a bond.
(424) |
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Term
|
Definition
Enthalpy is a state function
and is therefore
independent of path.
(429) |
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|
Term
|
Definition
Any quantity that depends solely
on the final destination,
not on
the way you get to that destination.
(429) |
|
|
Term
Enthalpy of formation
(ΔHf) |
|
Definition
The ΔH of
a formation reaction.
(430) |
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|
Term
What are standard enthalpies of formation? |
|
Definition
Standard conditions under which most chemistry is done:
- room temperature (25° Celsius)
- normal atmospheric pressure (1.00 atm)
(430) |
|
|
Term
In the symbol ΔHf0
what does the "0" tell you? |
|
Definition
That the enthalpy of formation
was measured
under standard conditons.
(430)
|
|
|
Term
What is the
standard enthalpy of formation
of an element in its elemental form? |
|
Definition
|
|
Term
|
Definition
Diagram that shows:
- the energy of the reactants
- intermediate state
- products in a chemical reaction.
(436) |
|
|
Term
|
Definition
Coordinate which tells
how close the reaction is to completion.
(436) |
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|
Term
|
Definition
A complex formed
in the process of a chemical reaction
when the reactants and products
are interacting.
(436) |
|
|
Term
|
Definition
Another name
for the intermediate state
of a chemical reaction.
(436) |
|
|
Term
|
Definition
The energy necessary
to start a chemical reaction.
(437) |
|
|
Term
|
Definition
A measure of
the disorder that exists in any system.
(437) |
|
|
Term
| Second Law of Thermodynamics |
|
Definition
The entropy of the universe must always either increase or remain the same.
It can never decrease.
(440) |
|
|
Term
What are
the relative entropy phases of matter?
(solid, liquid, gas)
|
|
Definition
- solid (least amount of entropy)
- liquid (greater amount of entropy)
- gas (highest amount of entropy)
(441) |
|
|
Term
With rising temperature,
the entropy of a system [increases/decreases]. |
|
Definition
|
|
Term
As the matter it contains increases,
the entropy of a system [increases/decreases. |
|
Definition
|
|
Term
Second Law of Thermodynamics
(mathematical equation) |
|
Definition
|
|
Term
All substances, even elements,
have ___________________. |
|
Definition
an absolute entropy.
(443) |
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|
Term
| Gibbs Free Energy (ΔG)formula |
|
Definition
|
|
Term
| Standard enthalpy of formation |
|
Definition
The ΔH of a formation reaction at
T = 298 K and P = 1.00 atm
(430) |
|
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Term
A reaction that is
consistent with the Second Law of Thermodynamics is said to be ____________. |
|
Definition
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|
Term
A reaction is called not spontaneous
when it is not consistent with the Second Law of Thermodynamics because ____________. |
|
Definition
the reaction cannot occur.
(446) |
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|
Term
When ΔG < 0,
then the reaction is
consistent with the Second Law,
and is therefore _____________. |
|
Definition
|
|
Term
If ΔG > 0,
then the reaction cannot proceed,
because it violates __________________. |
|
Definition
the Second Law of Thermodynamics.
(447) |
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