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IMU CET Kinetics — practice questions

Explore 71 free Kinetics questions in IMU CET Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Kinetics questions and exercises with answers

Showing questions 1–30 of 71.

Order the steps to find a rate lawRead the answer and worked solution →Fill in the reaction ordersRead the answer and worked solution →Complete the half-life rulesRead the answer and worked solution →Homogeneous or heterogeneous?Read the answer and worked solution →Elementary step or overall reaction?Read the answer and worked solution →Which is greater?Read the answer and worked solution →Which one does not belong?Read the answer and worked solution →Spot the false claimRead the answer and worked solution →Pop what speeds a reaction upRead the answer and worked solution →What does the rate of a chemical reaction measure?Read the answer and worked solution →For 2NH3 giving N2 plus 3H2, how does the rate of formation of hydrogen compare with the rate of formation of nitrogen?Read the answer and worked solution →Hydrogen peroxide decomposes as 2H2O2 giving 2H2O plus O2. If H2O2 disappears at 3.20 x 10^-2 mol/L/h, at what rate is O2 produced?Read the answer and worked solution →Which of these is not one of the five factors named as affecting reaction rate?Read the answer and worked solution →Small pieces of iron and of sodium are left exposed to air overnight. What is observed the next morning?Read the answer and worked solution →Phosphorus burns far more rapidly in pure oxygen than in ordinary air. Which factor explains this?Read the answer and worked solution →What is meant by the activation energy of a reaction?Read the answer and worked solution →Hydrogen peroxide foams on an open wound but keeps well in its bottle. Without catalysts, how long can complete decomposition take?Read the answer and worked solution →What does a rate law describe?Read the answer and worked solution →Which statement about the rate constant k is correct?Read the answer and worked solution →How are the exponents in a rate law obtained?Read the answer and worked solution →For rate = k[A]^2[B], what is the overall order of the reaction?Read the answer and worked solution →A reaction is second order in NO2 and zero order in CO. What is its rate law?Read the answer and worked solution →If a reaction is zero order with respect to one reactant, what does that tell you about that reactant?Read the answer and worked solution →With [O3] held fixed, doubling [NO] doubles the rate and tripling [NO] triples it. What is the order in NO?Read the answer and worked solution →For rate = k[NO][O3], a trial with [NO] = 1.00 x 10^-6 M and [O3] = 3.00 x 10^-6 M gives a rate of 6.60 x 10^-5 mol/L/s. What is k?Read the answer and worked solution →For rate = k[NO]^2[Cl2], a trial with [NO] = 0.10 M and [Cl2] = 0.10 M gives 0.00300 mol/L/s. What is k?Read the answer and worked solution →What units does the rate constant of a first order reaction carry?Read the answer and worked solution →What does an integrated rate law relate?Read the answer and worked solution →Which plot gives a straight line for a first order reaction?Read the answer and worked solution →Which plot gives a straight line for a simple second order reaction?Read the answer and worked solution →

Worked practice questions

Order the steps to find a rate law

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Steps
  1. Pick two trials
  2. Vary one reactant
  3. Compare rate ratio
  4. Read off the order
  5. Solve for k
Instructions
Tap the five steps in the order you would work through them.
_Source: OpenStax Chemistry, section 12.3 Rate Laws_

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Fill in the reaction orders

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Missing parts
  1. Answer
    second
    Choices
    1. first
    2. second
    3. zero
  2. Answer
    first
    Choices
    1. first
    2. second
    3. zero
  3. Answer
    third
    Choices
    1. second
    2. first
    3. third
Complete the statement
For rate = k[A]^2[B] the reaction is {0} order in A, {1} order in B, and {2} order overall.
Instructions
Tap the right order for each blank.
_Source: OpenStax Chemistry, section 12.3 Rate Laws_

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Complete the half-life rules

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Missing parts
  1. Answer
    0.693/k
    Choices
    1. 1/k
    2. k/0.693
    3. 0.693/k
  2. Answer
    5.02
    Choices
    1. 7.25
    2. 5.02
    3. 1.38
  3. Answer
    1/(k[A]0)
    Choices
    1. 1/(k[A]0)
    2. 0.693/k
    3. 2k/[A]0
Complete the statement
A first order half-life is {0}, so a decay with k = 0.138 per day halves in about {1} days. A second order half-life instead reads {2}.
Instructions
Tap the right entry for each blank.
_Source: OpenStax Chemistry, section 12.4 Integrated Rate Laws_

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