Kinetics Flashcards

1
Q

what is the rate of reaction

A

the time it takes for all the reactants to have been used up/all the products to have been formed

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2
Q

forumla for ROR

A

change/time

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3
Q

Factors that affect reaction rate

A
temperature
concentration
light
catalysts
pressure in gasesous reactants
surface area in solid reactants
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4
Q

where is the ROR the fastest

A

at the beginning of the reaction due to the higher concentration of reactants

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5
Q

what is the collision theory

A

According to the collision theory, reactions can only occur when:

  1. Reactants collide in the correct orientation.
  2. Reactants have the enough energy to form its products.
  • activation and suficent kinetic energy is required
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6
Q

what is activation energy

A

the minimum energy needed for a reaction to occur

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7
Q

what is the maxwell boltzmann distribution

A
  • range of energy/Users/mayrasalazar/Downloads/51c06e6ee4b0a49e8c8f47e6-aaronq-1371569791668-screen_shot_20120502_at_11212_pm1335978747666-2.png
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8
Q

what is average kinetic energy proportional to

A

temperature

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9
Q

what is a fruitful collision

A

a collision which results in a reaction,

more succesful collions= increase of rate in a reaction

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10
Q

what does the increase of reactants do

A

increase the rate as there is a higher number of successful collisions

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11
Q

How to make the ROR better in solids

A
  • decrease particle size, as only surface molecules react
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12
Q

how to make the ROR better in gaseous

A

increase concentration

ideal gas concentration

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13
Q

what does increasing the temperature do

A

increases the kinetic energy, increases the rate of reaction, increases fruitful collisions
- shifts distribution graph

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14
Q

what is a catalyst

A

a substance that increases the rate without reacting itself

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15
Q

What Happens During a Reaction

A

A chemical reaction is essentially involves two processes, bond breaking and bond forming. As mentioned in the Energetics chapter, particles tend to react to become more stable.

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16
Q

collision theory summary

A

Collision theory – reactions take place as a result of particles (atoms or molecules) colliding and then undergoing a reaction. Not all collisions cause reaction, however, even in a system where the reaction is spontaneous. The particles must have sufficient kinetic energy, and the correct orientation with respect to each other for the two to react. Even then, the transition state may revert to the reactant molecules instead of forming the product molecules.

17
Q

what is chemical kinetics

A

the study of the factors that affect the ROR