Name ________________________________
Quiz 5 (Chem 106) February 15, 2008
⎟
⎟
⎠
⎞
⎜
⎜
⎝
⎛−−=
212
111
ln TTR
E
k
ka A
TR
E
kaln
1
ln +
⎟
⎠
⎞
⎜
⎝
⎛
−=
Katm/molL08206.0KJ/mol314.8 ==R
1. For a hypothetical reaction, when the temperature was increased from 34.0°
to 49.0°C, the value of the rate constant was found to increase by a factor of
2.50. Calculate the activation energy (in kJ/mol) for this reaction.
Ea = ___________
2. The destruction of ozone, O3, proceeds by a two-step reaction mechanism.
The first of these steps is slower than the second.
1: O3 + NO NO2 + O2 rate1 = ____________________
2: NO2 + O NO + O2 rate2 = ____________________
net: ______________________________ rate = _____________________
(a) Write the rate laws for the two reaction steps.
(b) Write the overall (net) reaction for the destruction of ozone.
(c) Circle the rate determining step.
(d) Cross out the reaction step that has the higher activation energy.
(e) Write the rate law for the net reaction.
k1
k2
