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Homework 8: Kinetics

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    These homework problems are suggested and will not be turned in for review. However, answers will be available for them the following week by your class TAs. For more homework feel free to go to the Homework page.


    In the following decomposition reaction,

    \[2 N_2O_5 → 4 NO_2 + O_2\]

    oxygen gas is produced at the average rate of 9.1 × 10-4 mol · L-1 · s-1. Over the same period, what is the average rate of the following:

    1. the production of nitrogen dioxide
    2. the loss of nitrogen pentoxide


    Consider the following reaction:

    N2(g) + 3 H2(g) → 2 NH3(g)

    If the rate of loss of hydrogen gas is 0.03 mol · L-1· s-1, what is the rate of production of ammonia?


    Nitrogen monoxide reacts with hydrogen gas to produce nitrogen gas and water vapor. The mechanism is believed to be:

    Step 1: 2 NO → N2O2
    Step 2: N2O2 + H2 → N2O + H2O
    Step 3: N2O + H2 → N2 + H2O

    For this reaction find the following:

    • the overall balanced equation
    • any reaction intermediates


    Give two reasons why most molecular collisions do not lead to a reaction.


    An important function for managers is to determine the rate-determining steps in their business processes. In a certain fast-food restaurant, it takes 3 minutes to cook the food, 1.5 minutes to wrap the food, and 5 minutes to take the order and make change. How would a good manager assign the work to four employees?


    For the hypothetical reaction

    \[2A + 3B → 3C + 2D\]

    the following rate data were obtained in three experiments at the same temperature:

    Initial [A] Initial [B] Initial rate
    (mole liter-1) (mole liter-1') (moles of A consumed liter-1‘ sec-1)
    0.10 0.10 0.10
    0.20 0.10 0.40
    0.20 0.20 0.40
    1. Determine the experimental rate equation for the reaction.
    2. Calculate the specific rate constant, k.
    3. What is the rate of this reaction when [A] =0.30M and [B] = 0.30M?


    For the hypothetical reaction

    \[2A + B → 2C\]

    the following data were collected in three experiments at 25°C:

    Initial [A] Initial [B] Initial rate
    (mole liter-1) (mole liter-1) (moles of A consumed liter-1 sec-1)
    0.10 0.20 300
    0.30 0.40 3600
    0.30 0.80 14400
    1. What is the experimental rate equation for this reaction?
    2. Calculate the specific rate constant for this reaction.


    In the reaction

    \[2NO + Cl_2 → 2NOCl\]

    the reactants and products are gases at the temperature of the reaction. The following rate data were measured for three experiments:

    Initial p{NO} Initial p{Cl2} Initial rate
    (atm) (atm) (moles of A consumed atm sec-1)
    0.50 0.50 5.1 x 10-3
    1.0 1.0 4.0 x 10-2
    0.50 1.0 1.0 x 10-2
    1. From these data, write the rate equation for this gas reaction. What order is the reaction in NO, Cl2, and overall?
    2. Calculate the specific rate constant for this reaction.


    The reaction 2NO + O2 → 2NO2 is first order in oxygen pressure and second order in the pressure of nitric oxide. Write the rate expression.


    The reaction

    \[A + B + C → D + F\]

    was found to be zero order with respect to A. A solution of reactants A, B, and C was prepared with the following initial concentrations: 0.2M of A, 0.4M of B, and 0.6M of G. The concentration of A in this solution dropped to essentially zero in 5 min. A second solution was prepared with the following initial concentrations: 0.03M of A, 0.4M of B, and 0.6M of C. How long will it take for A to disappear?


    For the reaction

    \[2NO + H_2 → N_2O + H_2O\]

    the following experimental rate data are collected in three successive experiments at the same temperature:

    Initial [NO] Initial [H2] Initial rate
    (mole liter-1) (mole liter-1') (moles of A consumed liter-1‘ sec-1)
    0.60 0.37 0.18
    1.20 0.37 0.72
    1.20 0.74 1.44

    Using these experimental data, write the rate expression for the reaction.


    The reaction

    2HCrO4- + 3HSO3- + 5H+ → 2Cr3+ + 3SO42- + 5HQO

    follows the rate equation

    Rate = k[HCrO4-][HSO3-]2[H+]

    Why isn’t the rate proportional to the numbers of ions of each kind that are shown by the equation?


    The reaction SO2Cl2 —> SO2 + Cl2 is a first-order reaction with the rate constant k = 2.2 x 10-5 sec-1 at 320°C. What fraction of SO2CI2 is decomposed on heating at 320°C for 90 min?


    It often is said that, near room temperature, a reaction rate doubles if the temperature is increased by 10°C. Calculate the activation energy of a reaction whose fate exactly doubles between 27°C and 37°C.


    What is the activation energy for a reaction for which an increase in temperature from 20°C to 30°C exactly triples the rate constant?


    The following data give the temperature dependence of the rate constant for the reaction N2O4 → 2NO2 → 1/2O2. Plot the data and calculate the activation energy of the reaction.

    T(K) k (sec-1)
    273 7.87 x 10-7
    298 3.46 x 10-5
    308 1.35 x 10-4
    318 4.98 x 10-4
    328 1.50 x 10-3
    338 4.87 x 10-3


    Consider the reaction

    CH4 + Cl2 → CH3Cl + HCl (occurs under light)

    The mechanism is a chain reaction involving Cl atoms and CH3 radicals. Which of the following steps does not terminate this chain reaction?

    1. CH3 + Cl → CH3CI
    2. CH3 + HCl → CH4 + Cl
    3. CH3 + CH3 → C2H2
    4. Cl + Cl → Cl2

    Homework 8: Kinetics is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts.

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