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Lesson: The Arrhenius Equation

Worksheet • 6 Questions

Q1:

Hydrolysis of the sugar sucrose ( C H O 1 2 2 2 1 1 ) produces glucose and fructose. This first-order reaction has a rate constant of 2 . 1 0 × 1 0 s at 2 7 C and 8 . 5 0 × 1 0 s at 3 7 C .

Calculate the activation energy for this reaction, to three significant figures.

Calculate the rate constant for this reaction at 4 7 C , to two significant figures.

  • A 3 . 2 × 1 0 s−1
  • B 2 . 5 × 1 0 s−1
  • C 6 . 3 × 1 0 s−1
  • D 4 . 6 × 1 0 s−1
  • E 1 . 1 × 1 0 s−1

Estimate, to two significant figures, the time needed for the concentration of a 0.150 M sucrose solution to decrease to 1 . 6 5 × 1 0 M at 2 0 C .

  • A 2 . 1 × 1 0 days
  • B 9 . 2 × 1 0 days
  • C 7 . 6 × 1 0 days
  • D 5 . 0 × 1 0 days
  • E 1 . 9 × 1 0 days

Q2:

When the temperature increases from 3 0 C to 3 7 C , the rate of an enzyme-catalyzed reaction increases by a factor of 1.47. Calculate to 3 significant figures the activation energy for this reaction.

Q3:

A sample of hydrogen peroxide decomposes with a rate constant of 2 . 2 0 × 1 0 5 s−1 at 8 0 C and 5 . 6 5 × 1 0 7 s−1 at 3 5 C . Calculate to 3 significant figures the activation energy for this reaction.

Q4:

The rate constant for a reaction, 𝑘 , was measured over a range of reaction temperatures, 𝑇 . The data were plotted on a graph of l n 𝑘 against 1 𝑇 . What is the frequency (pre-exponential) factor for the reaction in terms of the gradient of the plot 𝑚 and the 𝑦 -intercept 𝑐 ?

  • A e 𝑐
  • B e 𝑚
  • C l n ( 𝑐 )
  • D l n ( 𝑚 )
  • E e 𝑐

Q5:

A sample of dinitrogen pentoxide ( N O ) 2 5 decomposes with a rate constant of 1.66 L/mol⋅s at 650 K and 7.39 L/mol⋅s at 700 K. Calculate to 3 significant figures the activation energy for this reaction.

Q6:

Butene can decompose to two molecules of ethene when heated. The rate constant for the decomposition reaction at 3 2 5 C is 6 . 1 0 × 1 0 8 s−1 and the activation energy is 261.0 kJ/mol. Estimate the frequency (pre-exponential) factor for the reaction, to 2 significant figures.

  • A 3 . 8 × 1 0 1 5 s−1
  • B 1 . 2 × 1 0 9 s−1
  • C 5 . 4 × 1 0 3 4 s−1
  • D 6 . 3 × 1 0 2 2 s−1
  • E 3 . 0 × 1 0 1 6 s−1
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