15. Chemical Kinetics

Rate Law

15. Chemical Kinetics

Rate Law

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Rate law and reaction order | Kinetics | AP Chemistry | Khan Academy

10:39

Rate law and reaction order | Kinetics | AP Chemistry | Khan Academy

Khan Academy Organic Chemistry

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How to Find the Rate Law and Rate Constant (k)

03:42

How to Find the Rate Law and Rate Constant (k)

14.2 Rate Laws | General Chemistry

Kinetics: Initial Rates and Integrated Rate Laws

Professor Dave Explains

Kinetics: Chemistry's Demolition Derby - Crash Course Chemistry #32

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Multiple Choice

Given the following chemical reaction, A → B. If the concentration of A is doubled the rate increases by a factor of 2.83, what is the order of the reaction with respect to A.

The data below were collected for the following reaction:CH₃Cl (g) + 3 Cl₂ (g) → CCl₄ (g) + 3 HCl (g)

Calculate the value and units for the rate constant k.

The concentration of N₂O was monitored at a constant temperature as a function of time for the reaction below.

N₂O (g) → N₂ (g) + ½ O₂ (g)

Reaction Time and Concentration of Nitrous Oxide
Time (s)	Molar Concentration [N₂O]
0	0.500 M
20	0.382 M
40	0.310 M
60	0.260 M
80	0.224 M

Determine the rate law for this reaction.

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Multiple Choice

Using the data below (also from questions 6 and 7), determine the value of the rate constant for the reaction.

Data Table for Three Experiments
Experiment	Initial [NH₄⁺]	Initial [NO₂]	Initial rate (M/s)
Experiment 1	0.24 M	0.10 M	7.2 × 10^-6 M/s
Experiment 2	0.12 M	0.10 M	3.6 × 10^-6 M/s
Experiment 3	0.12 M	0.15 M	5.4 × 10^-6 M/s

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Multiple Choice

For the reaction 2 NOCl (g) → 2 NO (g) + Cl₂ (g), the experimental rate law is: rate = k[NOCl]²[NO]^-1

Determine if the following mechanism is valid.

Step 1: NOCl (g) ⇌ NO (g) + Cl (g) (fast)

Step 2: NOCl (g) + Cl (g) → NO (g) + Cl₂ (g) (slow)

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Textbook Question

The following diagrams represent mixtures of NO(g) and O21g2. These two substances react as follows: 2 NO1g2 + O21g2¡2 NO21g2 It has been determined experimentally that the rate is second order in NO and first order in O2. Based on this fact, which of the following mixtures will have the fastest initial rate? [Section 14.3]

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Textbook Question

A reaction A + B¡C obeys the following rate law: Rate = k3B42. (a) If [A] is doubled, how will the rate change? Will the rate constant change?

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Textbook Question

A reaction A + B¡C obeys the following rate law: Rate = k3B42. (b) What are the reaction orders for A and B? What is the overall reaction order?

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Textbook Question

Consider a hypothetical reaction between A, B, and C that is first order in A, zero order in B, and second order in C. (e) By what factor does the rate change when the concentrations of all three reactants are tripled?

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Textbook Question

Consider a hypothetical reaction between A, B, and C that is first order in A, zero order in B, and second order in C. (a) Write the rate law for the reaction.

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Textbook Question

The decomposition reaction of N2O5 in carbon tetrachloride is 2 N2O5¡4 NO2 + O2. The rate law is first order in N2O5. At 64 C the rate constant is 4.82 * 10-3 s-1. (a) Write the rate law for the reaction.

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Textbook Question

Consider the following reaction: 2 NO1g2 + 2 H21g2¡N21g2 + 2 H2O1g2 (d) What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and 3H24 is increased to 0.030 M?

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Textbook Question

The react ion between ethyl bromide 1C2H5Br2 and hydroxide ion in ethyl alcohol at 330 K, C2H5Br1alc2 + OH- 1alc2¡ C2H5OH1l2 + Br - 1alc2, is first order each in ethyl bromide and hydroxide ion. When 3C2H5Br4 is 0.0477 M and 3OH- 4 is 0.100 M, the rate of disappearance of ethyl bromide is 1.7 * 10-7 M>s. (c) How would the rate of disappearance of ethyl bromide change if the solution were diluted by adding an equal volume of pure ethyl alcohol to the solution?

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl - + I - ¡OI - + Cl - . This rapid reaction gives the following rate data: 3oCl4 1M 2 3I4 1M 2 Initial Rate 1M,s2 1.5 * 10-3 1.5 * 10-3 1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4 1.5 * 10-3 3.0 * 10-3 2.72 * 10-4 (c) Calculate the rate when 3OCl-4 = 2.0 * 10-3 M and 3I - 4 = 5.0 * 10 - 4 M.

This graph shows a plot of the rate of a reaction versus the concentration of the reactant A for the reaction A ¡ products. a. What is the order of the reaction with respect to A?

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Textbook Question

The following data were measured for the reaction BF31g2 + NH31g2 ¡ F3BNH31g2: Experiment 3bF3 4 1M 2 3nH3 4 1M 2 Initial Rate 1M,s2 1 0.250 0.250 0.2130 2 0.250 0.125 0.1065 3 0.200 0.100 0.0682 4 0.350 0.100 0.1193 5 0.175 0.100 0.0596 (b) What is the overall order of the reaction?

This graph shows a plot of the rate of a reaction versus the concentration of the reactant A for the reaction A ¡ products. c. Write a rate law for the reaction including an estimate for the value of k.

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Textbook Question

This graph shows a plot of the rate of a reaction versus the concentration of the reactant. c. Write a rate law for the reaction including the value of k.

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Textbook Question

This graph shows a plot of the rate of a reaction versus the concentration of the reactant.

b. Make a rough sketch of a plot of [A] versus time

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Textbook Question

This graph shows a plot of the rate of a reaction versus the concentration of the reactant. a. What is the order of the reaction with respect to A?

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Textbook Question

Consider the gas-phase reaction between nitric oxide and bromine at 273 C: 2 NO1g2 + Br21g2¡2 NOBr1g2. The following data for the initial rate of appearance of NOBr were obtained: Experiment 3no4 1M 2 3br2 4 1M 2 Initial Rate 1M,s2 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 (b) Calculate the average value of the rate constant for the appearance of NOBr from the four data sets.

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Textbook Question

What are the units of k for each type of reaction? b. second-order reaction

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Textbook Question

This reaction is first order in N2O5: N2O5( g) ¡ NO3( g) + NO2( g) The rate constant for the reaction at a certain temperature is 0.053>s. a. Calculate the rate of the reaction when [N2O5] = 0.055 M

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Textbook Question

Consider the reaction of peroxydisulfate ion 1S2O82-2 with iodide ion 1I - 2 in aqueous solution: S2O8 2 - 1aq2 + 3 I - 1aq2¡2 SO42 - 1aq2 + I3- 1aq2 At a particular temperature, the initial rate of disappearance of S2O82 - varies with reactant concentrations in the following manner: Experiment 3S2o8 24 1M 2 3I4 1M 2 Initial Rate 1M,s2 1 0.018 0.036 2.6 * 10-6 2 0.027 0.036 3.9 * 10-6 3 0.036 0.054 7.8 * 10-6 4 0.050 0.072 1.4 * 10-5 (a) Determine the rate law for the reaction and state the units of the rate constant.

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Textbook Question

This reaction is first order in N2O5: N2O5( g) ¡ NO3( g) + NO2( g) The rate constant for the reaction at a certain temperature is 0.053>s. b. What would the rate of the reaction be at the concentration indicated in part a if the reaction were second order? Zero order? (Assume the same numerical value for the rate constant with the appropriate units.)

A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)?

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Textbook Question

A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C. b. What is the overall order of the reaction?

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Textbook Question

The following reaction is first order in A (red spheres) and first order in B (blue spheres): A + B¡Products Rate = k[A][B] (1)

(2)

(3)

(4)

(a) What are the relative rates of this reaction in vessels (1)–(4)? Each vessel has the same volume.

The following reaction is first order in A (red spheres) and first order in B (blue spheres): A + B¡Products Rate = k[A][B] (1)

(2)

(3)

(4)

(b) What are the relative values of the rate constant k for vessels (1)–(4)?

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Textbook Question

A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. a. Write a rate law for the reaction.

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Textbook Question

A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. e. By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?

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Textbook Question

The following pictures represent the progress of the reaction AS B in which A molecules (red spheres) are converted to B molecules (blue spheres).

(b) Draw a picture that shows the number of A and B molecules present at t = 3 min.

The following pictures represent the progress of the reaction AS B in which A molecules (red spheres) are converted to B molecules (blue spheres).

(c) Suppose that each sphere represents 6.0 * 1021 molecules and that the volume of the container is 1.0 L. What is the rate constant for the reaction in the usual units?

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Textbook Question

The following pictures represent the progress of a reaction in which two A molecules combine to give a more complex molecule A2, 2 AS A2.

(b) What is the rate law?

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Textbook Question

Consider the tabulated data showing the initial rate of a reaction (A ¡ products) at several different concentrations of A. What is the order of the reaction? Write a rate law for the reaction including the value of the rate constant, k.

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Textbook Question

The relative rates of the reaction A + B S AB in vessels (1)–(3) are 4:4:1. Red spheres represent A molecules, and blue spheres represent B molecules. (1)-(3)

(a) What is the order of the reaction in A and B?

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Textbook Question

The tabulated data were collected for this reaction: CH3Cl( g) + 3 Cl2( g) ¡ CCl4( g) + 3 HCl( g

Write an expression for the reaction rate law and calculate the value of the rate constant, k. What is the overall order of the reaction?

Consider a reaction that occurs by the following mechanism: A + BC SAC + B AC + D SA + CD The potential energy profile for this reaction is as follows:

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Textbook Question

The reaction 2NO1g2 + 2 H21g2S N21g2 + 2 H2O1g2 is first order in H2 and second order in NO. Write the rate law, and specify the units of the rate constant.

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Textbook Question

Initial rate data at 25 °C are listed in the table for the reaction NH4 +1aq2 + NO2 -1aq2S N21g2 + 2 H2O1l2 (b) What is the value of the rate constant?

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Textbook Question

Trimethylamine and chlorine dioxide react in water in an electron transfer reaction to form the trimethylamine cation and chlorite ion: 1CH323 N1aq2 + ClO21aq2 + H2O1l2S 1CH323 NH+1aq2 + ClO2 -1aq2 + OH-1aq2 Initial rate data obtained at 23 °C are listed in the following table.

(b) What would be the initial rate in an experiment with initial concentrations 31CH323 N4 = 4.2 * 10-2 M and 3ClO24 = 3.4 * 10-2 M?

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Textbook Question

Consider the reaction: 2 O3( g)¡3 O2( g) The rate law for this reaction is: Rate = k [O3]2 [O2] Suppose that a 1.0-L reaction vessel initially contains 1.0 mol of O3 and 1.0 mol of O2. What fraction of the O3 will have reacted when the rate falls to one-half of its initial value?

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Textbook Question

The following data were collected for the desturction of O3 by H (O3 + H → O2 + OH) at very low concentrations (b) Calculate the rate constant

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Textbook Question

Consider the reaction A + B¡C + D. Is each of the following statements true or false? (c) If the reaction is an elementary reaction, the rate law of the reverse reaction is first order.

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Textbook Question

Consider the reaction A + B¡C + D. Is each of the following statements true or false? (b) If the reaction is an elementary reaction, the rate law is second order.

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Textbook Question

The reaction 2 NO1g2 + O21g2¡2 NO21g2 is second order in NO and first order in O2. When 3NO4 = 0.040 M, and 3O24 = 0.035 M, the observed rate of disappearance of NO is 9.3 * 10-5 M>s. (c) What are the units of the rate constant?

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Textbook Question

The reaction 2 NO1g2 + O21g2¡2 NO21g2 is second order in NO and first order in O2. When 3NO4 = 0.040 M, and 3O24 = 0.035 M, the observed rate of disappearance of NO is 9.3 * 10-5 M>s. (b) What is the value of the rate constant?

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Textbook Question

Consider the following reaction between mercury(II) chloride and oxalate ion: 2 HgCl21aq2 + C2O4 2 - 1aq2¡2 Cl - 1aq2 + 2 CO21g2 + Hg2Cl21s2 The initial rate of this reaction was determined for several concentrations of HgCl2 and C2O4 2 -, and the following rate data were obtained for the rate of disappearance of C2O4 2 - : Experiment 3HgCl2 4 1M 2 3C2o4 24 1M 2 Rate 1M,s2 1 0.164 0.15 3.2 * 10-5 2 0.164 0.45 2.9 * 10-4 3 0.082 0.45 1.4 * 10-4 4 0.246 0.15 4.8 * 10-5 (c) What is the reaction rate when the initial concentration of HgCl2 is 0.100 M and that of C2O4 2- is 0.25 M if the temperature is the same as that used to obtain the data shown?

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Textbook Question

Concentration–time data for the conversion of A and B to D are listed in the following table.

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Textbook Question

Consider the following concentration–time data for the reaction of iodide ion and hypochlorite ion 1OCl-2. The products are chloride ion and hypoiodite ion 1OI-2.

(a) Write a balanced equation for the reaction.

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Textbook Question

Consider the following concentration–time data for the reaction of iodide ion and hypochlorite ion 1OCl-2. The products are chloride ion and hypoiodite ion 1OI-2.

(b) Determine the rate law, and calculate the value of the rate constant.

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Textbook Question

Consider the reversible, first-order interconversion of two molecules A and B: A kfkrB where kf = 3.0 * 10-3 s-1 is the rate constant for the forward reaction and kr = 1.0 * 10-3 s-1 is the rate constant for the reverse reaction. We'll see in Chapter 15 that a reaction does not go to completion but instead reaches a state of equilibrium with comparable concentrations of reactants and products if the rate constants kf and kr have comparable values. (b) Draw a qualitative graph that shows how the rates of the forward and reverse reactions vary with time.

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Textbook Question

Consider the reversible, first-order interconversion of two molecules A and B: A kfkrB where kf = 3.0 * 10-3 s-1 is the rate constant for the forward reaction and kr = 1.0 * 10-3 s-1 is the rate constant for the reverse reaction. We'll see in Chapter 15 that a reaction does not go to completion but instead reaches a state of equilibrium with comparable concentrations of reactants and products if the rate constants kf and kr have comparable values. (c) What are the relative concentrations of B and A when the rates of the forward and reverse reactions become equal?

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Textbook Question

Consider the reversible, first-order interconversion of two molecules A and B: A kfkrBwhere kf = 3.0 * 10-3 s-1 is the rate constant for the forward reaction and kr = 1.0 * 10-3 s-1 is the rate constant for the reverse reaction. We'll see in Chapter 15 that a reaction does not go to completion but instead reaches a state of equilibrium with comparable concentrations of reactants and products if the rate constants kf and kr have comparable values. (a) What are the rate laws for the forward and reverse reactions?

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Textbook Question

The following experimental data were obtained in a study of the reaction 2 HI1g2S H21g2 + I21g2. Predict the concentration of HI that would give a rate of 1.0 * 10-5 M>s at 650 K.

The rate constant for the first-order decomposition of gaseous N2O5 to NO2 and O2 is 1.7 * 10-3 s-1 at 55 °C. (b) Use the data in Appendix B to calculate the initial rate at which the reaction mixture absorbs heat (in J/s). You may assume that the heat of the reaction is independent of temperature.

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Textbook Question

You may have been told not to mix bleach and ammonia. The reason is that bleach (sodium hypochlorite) reacts with ammonia to produce toxic chloramines, such as NH2Cl. For example, in basic solution: OCl-1aq2 + NH31aq2S OH-1aq2 + NH2Cl1aq2 (a) The following initial rate data for this reaction were obtained in basic solution at 25 °C

What is the rate law for the reaction? What is the numerical value of the rate constant k, including the correct units?

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Open Question

Consider the rate law. rate=𝑘[a]^𝑥 determine the value of 𝑥 if the rate doubles when [a] is doubled.

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Open Question

Using the data in the table, determine the rate constant of the reaction and select the appropriate units. a+2b⟶c+d

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Open Question

Using the data in the table, calculate the rate constant of this reaction. a+b⟶c+d

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Open Question

For each reaction order, identify the proper units for the rate constant, 𝑘. not all of the choices will be used.

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Open Question

What is the value of the rate constant k for this reaction?

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Open Question

Consider the rate law. Rate = k[A]^x. Determine the value of x if the rate doubles when [A] is doubled.

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Open Question

According to this data, what is the order of the reaction in OH^-, to the nearest whole number?

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Open Question

Considering the rate law, rate = k[a]²[b], which of the following statements is correct?

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Open Question

Consider the following reaction: 2 Mg + O₂ → 2 MgO, rate=k[Mg][O₂]²

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Open Question

Determine the rate law for each elementary step. drag the symbols into the equations as needed.

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Open Question

Calculate the initial rate for the formation of c at 25 °C, if [A] = 0.50 M and [B] = 0.075 M.

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Open Question

What is the rate law for the reaction A → B if the rate constant, k, is 0.25 m^-1 s^-1 at 75 °C?

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Open Question

Consider the rate constants below. Which would correspond to the highest order reaction?

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Open Question

If the reaction X + 2 Y → XY₂ occurs by the proposed mechanism, what is the rate law?

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Open Question

If a rate law is second order (reactant), doubling the reactant ________ the reaction rate.

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Multiple Choice

In the experiments on the reaction 2 ICl (g) + H₂ (g) → I₂ (g) + 2 HCl (g), the following initial rate data were obtained. What is the overall order of the reaction?

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Rate Law

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