Docsity
Docsity

Prepare for your exams
Prepare for your exams

Study with the several resources on Docsity


Earn points to download
Earn points to download

Earn points by helping other students or get them with a premium plan


Guidelines and tips
Guidelines and tips

Calculate Activation Energy, Rate Determining Step - Quiz 5 | CHEM 106, Quizzes of Chemistry

Material Type: Quiz; Professor: Glendening; Class: Gen Chemistry II; Subject: Chemistry; University: Indiana State University; Term: Spring 2008;

Typology: Quizzes

Pre 2010

Uploaded on 07/23/2009

koofers-user-0qz
koofers-user-0qz 🇺🇸

10 documents

1 / 1

Toggle sidebar

This page cannot be seen from the preview

Don't miss anything!

bg1
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

Partial preview of the text

Download Calculate Activation Energy, Rate Determining Step - Quiz 5 | CHEM 106 and more Quizzes Chemistry in PDF only on Docsity!

_Name _________________________________

Quiz 5 (Chem 106) February 15, 2008

2 1 2

ln 1 1 1 R T T

E

k

k (^) a A R T

E

k a^ ln

ln (^) ⎟ + ⎠

R = 8. 314 J/molK = 0. 08206 Latm/mol K

  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.

E a = ___________

  1. The destruction of ozone, O 3 , proceeds by a two-step reaction mechanism. The first of these steps is slower than the second.

1: O 3 + NO NO 2 + O 2 rate 1 = ____________________

2: NO 2 + O NO + O 2 rate 2 = ____________________

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.

k 1

k 2