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kinetics and equilibrium
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Cards (83)
What is the activation energy (EA)?
Minimum
energy
needed
for a
reaction
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What does the Maxwell-Boltzmann energy distribution illustrate?
Spread of energies in
gas or liquid
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Why does the energy distribution curve go through the origin?
No
molecules
have zero energy
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Why does the energy distribution curve never meet the x-axis?
No maximum energy for
molecules
exists
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Where is the mean energy of particles located on the curve?
Not
at
the
peak
of
the
curve
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What does the area under the Maxwell-Boltzmann curve represent?
Total number of
particles
present
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Why do a few particles have low energies?
Collisions
cause some particles to slow down
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How can a reaction go to completion if few particles exceed EA?
Particles can gain energy through
collisions
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What does Emp represent in the energy distribution?
Most probable energy of
particles
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What happens to the energy distribution as temperature increases?
More
molecules
have higher energies
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What remains constant as temperature increases?
Total area under the
curve
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How does the range of energies change with temperature?
Wider
range of energies at
higher
temperatures
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What happens to Emp and mean energy at higher temperatures?
Both
shift to
higher
energy values
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What is the rate of reaction defined as?
Change in
concentration
over
time
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How is the rate of reaction determined from a concentration vs. time graph?
Gradient
of the curve indicates rate
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What is the initial rate of reaction?
Rate
at the
start
of the reaction
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How can reaction rates be calculated from graphs?
By drawing a tangent and calculating
gradient
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What effect does increasing concentration have on particle collisions?
Increases frequency of
effective collisions
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How does the shape of energy distribution curves change with concentration?
Curves become higher,
area
increases
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What happens to the number of molecules with energy > EA when concentration increases?
More molecules exceed
activation energy
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What state do all reversible reactions reach?
Dynamic equilibrium state
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How do different volumes of the same initial concentrations affect reaction rates?
Same
initial rate, different
final
amounts
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What is the general reaction for the formation of ammonia?
N2
+
3H2
⇌
2NH3
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What are the two features of dynamic equilibrium?
Forward
and
backward
reactions occur at
equal rates
.
Concentrations
of reactants and products remain constant.
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What factors increase the rate of reaction?
Higher
concentration
,
temperature
,
surface area
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What does the term 'position of equilibrium' refer to?
Composition of the
equilibrium mixture
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How is the reaction rate measured in the sodium thiosulfate and hydrochloric acid experiment?
As 1/
time
for cross disappearance
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What happens if the position of equilibrium favors the reactants?
Equilibrium mixture
contains mostly reactants
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Why is measuring 1/time an approximation for reaction rate?
It does not include
concentration changes
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What does Le Chatelier’s principle state?
If an external condition changes,
equilibrium
shifts to oppose the change.
It tries to reverse the effect of the change.
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How does increasing temperature affect equilibrium?
Shifts to
endothermic
direction to absorb heat
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What happens when concentration is doubled?
Double the number of
particles
per volume
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What is the effect of increasing temperature on ammonia yield?
Lower
yield
of
ammonia
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How does increasing surface area affect reaction rates?
Increases frequency of
successful collisions
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What happens if temperature is decreased in a reaction?
Equilibrium
shifts to exothermic direction
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What is the definition of a catalyst?
Increases
reaction
rates without being used
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What is the trade-off with low temperatures in reactions?
Higher
yield
but slower
reaction rates
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How does increasing pressure affect equilibrium?
Shifts towards side with fewer
moles
of
gas
.
Reduces pressure by opposing the change.
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How do catalysts increase reaction rates?
By providing an alternative route with lower
EA
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What is the effect of increasing pressure on methanol yield?
Higher
yield of
methanol
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See all 83 cards
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