# Notes taken during lecture

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31 Dec 2010
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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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## Document Summary

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 . When pressure and temperature cannot be readily controlled, a enzyme allows reactions to occur under relatively mild conditions do not need to know mechanism. 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. Making reactants at same rate as products past the dotted vertical line, chemical equilibrium achieved same rate. Once at equilibrium, colour will not change because relative concentrations will not change. Ans:c note exponent 2 from coefficient of no2 because of arrhenius equation no units. Rt to the power of (c+d-a-b) is basically rt to the power of delta n www. notesolution. com. Concentration depend on amount of co2, not any of the solids.

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