3.1.5 Kinetics Flashcards
define collision theory
particles must collide with sufficient energy and correct orientation in order for a reaction to take place.
define activation energy
the minimum amount of kinetic energy particles must have in order to react
what is the rate of reaction
the frequency of successful collisions
what goes on the x axis on Maxwell distribution curve
Energy
what goes on the y axis
number of molecules with energy
on M-D curve where is the most probably energy
peak of curve
on M-D curve why is the most probable energy not the same as mean energy
particles with very high energy skew average
where does M-D curve start and why
at 0,0 because no molecules have o energy
When does M-D curve cross x axis
it doesn’t it is an asymptote
because no limit to maximum energy particles can have
what does the area under M-D curve represent
the area is equal to the total number of molecules
what does a catalyst do
Increased the rate of reaction by providing an alternate reaction route with lower activation energy and is not changed in chemical composition or amount
what is a homogeneous catalyst
it is in the same phase as the reactants
what is a heterogeneous catalysts
it is in a different state to the reactants
why does a catalyst increase rate of reaction explain in relation to M-D curve
A greater proportion of molecules have sufficient energy this increases the frequency of successful collisions
what happens to M-D curve when temperature increases
x5 points
peak to the right
Peak lower
crosses old curve one
same area
end above the old one
effect of increasing concentration on rate of reaction
increases the frequency of successful collisions
What happens to M-D curve when pressure increase
Nothing
Because particles still collide with the same amount of energy
Rate equation
(Amount of reactant used or product made) / time
What happens to M-D curve when you decrease the temperature x5 points
Shifts to the left
Peak is higher
Area is the same
End line is under the original
Crosses once
Why is rate of reaction faster when temperature is increased
Particles have more kinetic energy so there is a higher frequency of successful collisions
What effect would increasing the pressure have on rate of reaction and why
Increasing pressure increases the rate of reaction
Because particles are more close together there is a higher frequency of successful collisions
How does increasing concentration effect reaction and why
Increasing concentration increases the rate of reaction
The particles are closer together so there is a higher frequency of successful collisions
For M-D curve which if these is it Molecules, Particles, Atoms
Must be MOLECULES
Why is SO2 bad to reduce in classroom experiment
Toxic
Is the average kinetic energy of molecules in a gas constant?
Yes
