Quiz 2 Flashcards
The higher the reaction barrier(activation energy)
the slower the reaction
reactions at higher temperatures
are faster reactions becasue
* molecules colide more frequently
* molecules collide with more energy
Measuring intial rate
- slope of line at start of reaction
rise/run - 10-15% of the reaction progress
Average reaction rate
(final consentration-inital consentration)/(final time- inital time)
Calculating order
Zero-order rate constant unit
M s^-1
First-order rate constant unit
s^-1
Second-order rate constant unit
M^-1 s^-1
Integrated Rate Law graph
Zero Order
Integrated Rate Law graph
First Order
Integrated Rate Law graph
Second Order
mechanism of a reaction
the detailed stepwise process of how we get from starting materials to the products
Ea
“energy barrier to reaction”
Activation energy
Large Ea
slow reaction
Small Ea
Fast reaction
ΔH
ΔE = change in energy
product energy - reactants energy
ΔH < 0
favorable reaction
ΔH > 0
Unfavorable reaction
In reactions catalysts
lower the activation energy (lowers hump)
k= rate constant
A= frequency factor
Ea= activation energy
R= gas constant
T= temperature in kelvin
parts of arrhenius equation
calculating Ea
Ea= slope of equation x R
calculating A
comparing activation energy at diff temps
