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Department
Chemistry
Course Code
CHM135H1
Professor
Kris Quinlan

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LECTURE 8: Kinetics and Equilibrium
Slide No. Notes
KINETICS
31 -lower to higher temperature, energy of collisions increases
-for a reaction to occur, there must be a collision and the collision
must have sufficient energy
35 -increasing temperature, the smaller the exponent, therefore the
larger the k
-to use the equation, either get data from two different temperature
points to determine activation energy or graphically
37 - Ea = -Rin(k2/k1) all over (1/T2 – 1/T1) = -8.314J/molK times
In(1.10x10^-5L/mols divided by 9.51x10^-9L/mols) all over (1/600K
1/500K) = 1.76 kJ/mol
38 -valley – intermediates
-peaks – steps of the reaction
-a reaction is faster because the activation energy is smaller
-the energy difference between reactants and products remains
unchanged with a catalyst
-catalyst is at the beginning and end
-intermediate only at the middle, used up, not remade
40 - how a catalytic converter works
41 -when pressure and temperature cannot be readily controlled, a
enzyme allows reactions to occur under relatively mild conditions
-do not need to know mechanism
42 -Ans1: B – compare 1 and 2 – double red, double rate – first order
-Ans2: A – compare 1 and 3 – double blue, no change in rate – 0th
order
-Ans3: B – any concentration that affects rate of reaction does not
have to be in final equation
-Compare 1 and 4
-Therefore rate = k[A][C]
EQUILIB.
2-making reactants at same rate as products
-past the dotted vertical line, chemical equilibrium achieved – same
rate
3- once at equilibrium, colour will not change because relative concentrations
will not change
5- Ans:C
6-note exponent 2 – from coefficient of NO2
-because of Arrhenius equation
7-no units
-Ans: A
8-RT to the power of (c+d-a-b) is basically RT to the power of delta n
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Description
LECTURE 8: Kinetics and Equilibrium Slide No. Notes KINETICS 31 - lower to higher temperature, energy of collisions increases - for a reaction to occur, there must be a collision and the collision must have sufficient energy 35 - increasing temperature, the smaller the exponent, therefore the larger the k - to use the equation, either get data from two different temperature points to determine activation energy or graphically 37 - Ea = -Rin(k2k1) all over (1T2 1T1) = -8.314JmolK times In(1.10x10^-5Lmols divided by 9.51x10^-9Lmols) all over (1600K 1500K) = 1.76 kJmol 38 - valley intermediates - peaks steps of the reaction - a reaction is faster because the activation energy is smaller - the energy difference between reactants and products remains unchanged with a catalyst - catalyst is at the beginning and end - intermediate only at the middle, used up, not remade 40 - how a catalytic converter works 41 - when pressure and temperature cannot be readi
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