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#9 Writing and Interpreting a Rate Law Expression 1. The gas phase reaction of nitric oxide...

#9 Writing and Interpreting a Rate Law Expression

1. The gas phase reaction of nitric oxide and oxygen yields nitrogen dioxide:

2 NO (g) + O₂ (g) ----> 2 NO₂ (g)

The rate law is rate = k[NO]²[O₂].

a. What is the reaction order with respect to each reactant and what is the overall reaction order?

b. What are the units for k if time was expressed in units of minutes?

c. If the concentration of NO was doubled and the concentration of O₂ was halved, what would happen to the rate?

d. If the NO was unchanged and the concentration of O₂ was doubled, what would happen to the rate?

e. If both of the reactants were tripled, what would happen to the rate?

2. The reaction…

2 ICl (g) + H₂ (g) ------> I₂ (g) + 2 HCl (g)

is first order in H₂ and first order in ICl. Write the rate law expression and specify the units of the rate constant, k.

3. The reaction of CO and NO₂ is second order with respect to NO₂ and zero order with respect to CO.

a. Write the rate law expression.

b. Expressing time in units of seconds, what are the units for k?

c. How does the reaction rate change if the CO concentration is decreased by a factor of 5?

d. What is the change in the rate if the concentrations of both reactants is doubled?

4. Using time units of hours, what would the units for k be for a reaction that is 1½ order?

5. For the following rate law…

Rate = k[NO₂]²[H₂]

a. What is the order with respect to each reactant?

b. What is the overall order for the reaction?

c. What are the units for the rate constant, k, if the time unit is seconds?

d. What would happen to the rate if each reactant was quadrupled?

e. What would happen to the rate if NO₂ was unchanged and the H₂ was halved?

Expert Solution

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queen_honey_blossom answered 4 months ago

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