# Kinetics WS

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```					      Chemistry Kinetics – Practice

Collision & Kinetic Theory
1. Sketch a Potential Energy diagram for a reaction with a two step mechanism. The
second step is the rate-determining step.
Label the axes.
The overall activation energy is about 80 kJ/mole, while around 20 kJ/mole are released
as the products form.
Show on the diagram the H, the Ea, the location of the intermediates and transition
states (if any), the reactants and the products.

Energy, (kJ/mol)

Reaction progress (time)

2. Which of the reactions below will have a higher reaction rate? Explain:

Energy, (kJ/mol)

Reaction progress (time)                       Reaction progress (time)
Chemistry Kinetics – Practice

Rate of Reaction
3. When starting a reaction, the concentration of one of the reagents was 1.50 M. After
three minutes, the concentration of this reagent was 0.85 M. Using these data, determine
the average rate of this reaction in M/sec.

4. Using the rate equation, Rate = k [A]2[B], define the order of the reaction with respect to
A and B. What is the total order of the reaction?
order w/r [A] = ______           order w/r [B] = ______       overall order = _____

5. Find the rate law for the following reactions using the concentration/rate data:

6. Nitrogen monoxide gas and hydrogen gas react according to the rate law:
Rate = k[NO]2[H2]
How does the rate change if:
(a) the concentration of hydrogen is doubled.
(b) the concentration of nitrogen monoxide is doubled.
(c) the concentration of hydrogen is cut in half.
(d) the volume of the container is cut in half.
(e) the temperature is increased.

```
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