Integrated Rate Laws

X → products

Pure substance X decomposes according to the equation above. Which of the following graphs indicates that the rate of decomposition is second order in X ?

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• 
• 

Which of the following best identifies the rate constant k

for the reaction based on the information in the plot of ln[H₂O₂] versus time (t) ?

• k = ln[H₂O₂] at t=0s

• k = −(slope of plot)

• k = ln[H₂O₂] at t=500s

What is the rate constant for a first-order reaction with an initial reactant concentration of .300 mol/L if, after 200 s, the concentration is .200 mol/L?

• .005 s^-1

• .002 s^-1

• .001 s^-1

• .006 s^-1

The graphs shown in the diagram indicate that reactant A is ________________ order.

• zero

• first

• second

Given the following differential rate late, what be the units for k?

Rate = k[A][B]²

• 1/M s

• 1/M² s

• 1/M³ s

• 1/s

What is the order with respect to A according to the graphs of data?

• zero

• first

• second

• no way to tell

The reaction is _________ order with respect to N₂O_2.

• zeroeth

• first

• second

• half

Which equation below would be used to find the concentration of reactant [A] at a specific time for a reaction with the following rate law? rate = k[A]

• ln [A] = -kt + ln[A]₀

• 1/[A] = kt + 1/[A]₀

• [A] = - kt + [A]₀

What rate order is demonstrated by the diagram for reactant A?

• zero order

• first order

• second order

Given the following data for the decomposition of NO₂:

2 NO₂ --> 2 NO + O₂

Time(s) [NO₂] (M)

0.0 0.100

5.0 0.017

10.0 0.0090

15.0 0.0062

20.0 0.0047

What is the order of this reaction

• zero order

• 1st order

• 2nd order

• 3rd order