FINAL - SECTION 5 Flashcards
Reaction rate
Represented as [ ]/T and measures how fast concentration is (concentration and time)
+ sign
Product
- sign
Reactant
What do you do with the mole quantity
Put it at the bottom of fraction in equation
Unit of reaction rate
M/S
Differential rate law
Measures rate and concentration
Rate law
k[A]^n
Zero order
Rate is constant and independant on concentration (k[A]^0)
First order
Rate is dependant on concentration ( k[A]^1) and 2x
Second order
Rate is dependant on concentration (k[A]^2) and 4x
Units of k
- Zero order: M L s-1
- First order: s-1
- Second order: L M-1 s-1
Multiple rate reaction
Overall order becomes the sum of reactant exponents ( rate = k[A]^m[A]^n, overall order is m+n)
Integrated rate law
Concentration and time
What do we do with minutes in integrated rate law
Convert to seconds
“Plot of inverse”
Second order
What does [A]0 mean
Initial concentration
Kinetic graph interpretation
Whichever graph is most linear is what the order is ([A] vs time, ln[A], or 1/[A])
Half life
How long it takes for half the reactants to be consumed
Collision theory
Reactants must collide to reactant (higher concentration = higher probability)
Activation energy
Minimum energy needed for molecules to collide
H+
Endothermic (absorb)
H-
Exothermic (release)
Transition state
Top of energy curve
Arrhenius equation
Relate reaction and temperature
Reaction mechanism
Sequence of elementary steps by which a chemical reaction occurs
What happens to the moles in reaction mechanism
You can make it into a power (eg. 2NO + Cl = 2NOCl = k[NO]^2[Cl]
Catalyst
Increase rate of reaction by decreasing activation energy
Homogenous catalyst
Same phase as reactant
Heterogenous catalyst
Different phase as reactant
