AP Chem RQ 4

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 ?

• 
• 
• 
• 

Which of the following procedures will allow the student to determine the rate constant, k , for the reaction?

• Plot ln [X] versus time and determine the magnitude of the slope.

• Plot 1/[X] versus time and determine the magnitude of

  the slope.

• Run another trial of the experiment with a different initial concentration, plot the data on the same graph, and see where the curves intersect.

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 following integrated rate law could be used to find the the concentration of a ________________ order reactant at a certain time.

[A] = - kt + [A]₀

• zero

• first

• second

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

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

Given: CH₃COCH₃ + Cl₂ -> CH₃COCH₂Cl + HCl

The given reaction is zero order with respect to Cl₂ and first order with respect to CH₃COCH₃. Determine the concentration of CH₃COCH₃ after 30 seconds if the initial concentration of CH₃COCH₃ is 0.025 M and the rate constant at 25 ^oC is 1.32 x 10^-1 s^-1.

• 4.77 x 10^-4 M

• 4.77 x 10^-2 M

• 4.77 x 10^-3 M

• 4.77 x 10^-6 M

NO₂(g) → NO(g) + ½ O₂(g)

The graph of data for time vs. ln [NO₂] was a straight line with a negative slope. Which of the following would be the differential rate law for this reaction?

• rate = k[NO₂]

• rate = k[NO₂]²

• rate = k