Ch.13 - Chemical KineticsWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Sections
Rate of Reaction
Average Rate of Reaction
Arrhenius Equation
Rate Law
Integrated Rate Law
Collision Theory
Additional Practice
Instantaneous Rate of Change
Energy Diagram
Catalyst
Michaelis-Menten Equation
Reaction Mechanism
Identifying Reaction Order
LearnAdditional PracticeSummary
Next SectionIntegrated Rate Law

Rate Law represents an equation for a chemical reaction that connects the reaction rate with the concentrations or pressures of the reactants and the rate constant. 

Rate Law

When it comes to the rate of a reaction the Rate Law focuses on the reactant concentrations, while ignoring the product concentrations. 

Concept #1: Understanding the Rate Law. 

By focusing on only the reactant concentrations we only care about the forward direction of our chemical reaction. 

Concept #2: The Rate Determining Step. 

If the reaction says it’s a SLOW step or a ONE-STEP MECHANISM then we can simply look at the coefficients of the reactants to determine the reaction orders. 

Example #1: For the following reaction, use the given rate law to determine the best answer for the reaction with respect to each reactant and the overall order.

H2O2 (aq) + 3 I – (aq) + 2 H+ (aq)  --->  I3 – + 2 H2O (l)  

 

Rate = k [H2O2]2 [I –]

 

a) H2O2 is 1st order, I – is 1st order, 2nd order overall.

b) H2O2 is 2nd order, I – is 1st order, 3nd order overall.

c) H2O2 is 0th order, I – is 1st order, H+ is 1st order, 3rd order overall.

d) H2O2 is 2nd order, I – is 1st order, H+ is 0th order, 3rd order overall.

Example #2: Answer each of the following question based on the following chemical reaction:

Calculate the reaction order for reactant A. 

Practice: Calculate the reaction orders for Reactants B and C.

Example #3: Calculate the rate constant and the new rate for the given reaction if the initial concentration of [A] = 0.300 M, [B] = 0.150 M and [C] = 0.150 M.

The Rate Constant k

The Rate Constant k can have a direct impact on the rate of the reaction. In order to determine its units just utilize the equation below, where n is the overall order of the reaction: 

Example #4: A certain chemical reaction has the given rate law:

Rate = k [A]3 [B]2 [C]-1

What are the units of the rate constant for the given reaction?

a) M-2 s-1      b) M2 s-1       c) M-4 s-1      d) M-3 s-1      e) M3 s-1

Example #5: The reaction of 3 A + B ---> 2 C + D, was found to be: Rate = k [A]2 [B]3. How much would the rate increase by if A were tripled while B were increased by half?

a) 0.50              b) 30.38            c) 0.75              d) 20.25            e) 1.125

Practice: If the rate law for the following reaction is found to be the following, what are the units for the rate constant, K?

Cl2 (g) + HCCl3 (g) → HCl (g) + CCl4 (g)

a)          b)           c)           d)           e) 

Reaction Mechanisms

Concept #3: A   Reaction Mechanism   involves a series of elementary reactions that give the overall equation. 

Previous SectionArrhenius Equation
Next SectionIntegrated Rate Law
Additional Problems
Consider a reaction with the following rate law Rate = k [C]2[D]3[E]-1 By what factor would the rate of the reaction increase if the concentration of [C] tripled, the concentration of D is increased by half and concentration of [E] doubled? A. 15.2 B. 12.9 C. 9.0 D. 6.5 E. 30.4
 The rate law for a reaction is Rate = k[A][B]2 Which one of the following statements is false? a. The reaction is second order in respect to B.  b. If [B] is doubled, the reaction rate will increase by a factor of 4. c. If [A] is doubled, the reaction rate will increase by a factor of 2. d. The reaction is first order overall. 
Determine the rate law for the reaction 2ClO2 (aq) + 2 OH - (aq) → ClO2- + H2O (l) given the following data. a. Rate = k[ClO2][OH-] b. Rate = k[ClO2]2[OH-] c. Rate = k[ClO2]2[OH-]2 d. Rate = k[ClO2][OH-]2 e. Rate = k[OH-]
Consider the reaction A + B + C → products. It has the rate law rate = k[A]  -1[B]3[C]2 Which of the following statements(s) is/are correct? i. The units of the rate constant are M -3 time-1. ii. The overall order of the reaction is 5. iii. Increasing the concentration of A by a factor of 3, B by a factor of 2 and C by a factor of 4 results in the overall rate increasing by a factor of 42.7. A. i only B. ii only C. iii only D. i and iii E. ii and iii
The rate law for the reaction H2O2 + 2H+ + 2l- → I2 + 2H2O is rate = k [H2O2] [I-]. the overall order of the reaction is (A) five (B) three (C) two (D) one
The reaction of peroxydisulfate ion (S2O8 2- ) with iodide ion (I - ) is: S2O8 2- (aq) + 3I - (aq) → 2SO4 2- (aq) + I3 - (aq) a.) What is the rate law?     b.) What is the rate constant?          
The reaction of peroxydisulfate ion (S2O82‐) with Iodide ion (I1‐) S2O82–+ 3 I –(aq) → 2SO42– + I3 From the data below calculate the rate constant for the reaction, k. A) 0.143 B) 0.0049 C) 0.0115 D) 0.061 E) 0.337  
Consider this reaction and its rate law. 3A + 2B --> products rate = k[A][B] What is the order with respect to A? What is the order with respect to B? What is the overall reaction order?
Give the characteristic of a first order reaction having only one reactant.  A. The rate of the reaction is not proportional to the concentration of the reactant. B. The rate of the reaction is proportional to the square of the concentration of the reactant. C. The rate of the reaction is proportional to the square root of the concentration of the reactant. D. The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant.  E. The rate of the reaction is directly proportional to the concentration of the reactant. 
What is the overall order of the following reaction, given the rate law? 2NO(g) + H2(g) → N2(g) + 2H2O(g) Rate = k [NO]2[H2] A. 1st order B. 2nd order C. 3rd order D. 4th order E. 0th order
What are the units of k in the following rate law? A. Rate = k[X][Y]2 A) 1/Ms2 B) 1/M2s C) M2s D) M2/s E) 1/M3s
Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? A. Rate = k[X]2[Y]3 A) The rate of reaction will increase by a factor of 9. B) The rate of reaction will increase by a factor of 2. C) The rate of reaction will increase by a factor of 8. D) The rate of reaction will increase by a factor of 4. E) The rate of reaction will remain unchanged.
Determine the rate law and the value of k for the following reaction using the data providded. CO(g) + Cl2(g) → COCl2(g) [CO]i(M) [Cl2]i(M) Initial Rate (M-1s-1) 0.25         0.40             0.696 0.25         0.80             1.97 0.50         0.80             3.94 A) Rate = 11 M-3/2s-1[CO][Cl2]3/2 B) Rate = 36 M-1.8s-1[CO][Cl2]2.8 C) Rate = 17 M-2s-1[CO][Cl2]2 D) Rate = 4.4 M-1/2s-1[CO][Cl2]1/2 E) Rate = 18 M-3/2s-1[CO]2[Cl2]1/2  
Consult the table and find the rate constant of the reaction. A) 2.1 x 10-2 M-1 s-1 B) 2.1 x 10-1 M-1 s-1 C) 2.3 x 10-2 M-1 s-1 D) 1.4 x 10-1 M-1 s-1 E) 6.9 x 10-2 M-1 s-1
The reaction between ethyl bromide (C2H5Br) and hydroxide ion (OH -) in ethyl alcohol at 330 K is first order each in ethyl bromide and hydroxide ion. C2H5Br(alc) + OH -(alc) → C2H5OH(I) + Br -(alc) How would the rate of ethyl bromide change if the solution were diluted by adding an equal volume of pure ethyl alcohol to the solution.   a) no change b) decrease by a factor of four c) increase by a factor of four d) increase by a factor of two e) decrease by a factor of two
If the rate of a reaction increases by a factor of 9 when the concentration of reactant increases by a factor of 3, the order of the reaction (with respect to this reactant) is a) 2 b) 3 c) 9 d) 4 e) 1 
Given that the rate law for the production of water 2 H2 (g) +  O2 (g) → 2 H2O (l) is rate = k[H2]2[O2] –1, then the overall order of the reaction is  a) 1 b) 2 c) 3 d) –1 e) 0  
For the reaction 2A + B → products determine the rate law for the reaction given the following data:  Initial Concentration M,           Initial Rate, M·s–1   A          B 0.10       0.10                           2.0 x 10   –2 0.20       0.10                           8.0 x 10   –2 0.30       0.10                           1.8 x 10   –1 0.20       0.20                           8.0 x 10   –2 0.30       0.30                           1.8 x 10   –1 a) rate = k [A] b) rate = k [A][B] c) rate = k[A] [B] 0 d) rate = k[A]2 e) rate = k[B]2
When the reaction CH3Cl(g) + H2O(g) → CH3OH(g) + HCl(g) was studied, the tabulated data were obtained. Based on these data, what are the reaction orders? (A) CH3Cl: first order         H 2O: first order (B) CH3Cl: first order         H 2O: second order (C) CH3Cl: second order     H 2O: first order (D) CH3Cl: second order     H 2O: second order
The gas-phase reaction, A2 + B2 → 2AB, proceeds by bimolecular collisions between A2 and B2 molecules. If the concentrations of both A2 and B2 are doubled, the reaction rate will change by a factor of A) 1/2 B) √2 C) 2 D) 4
The following kinetic data was obtained for the reaction 2A + B → Products
Initial rate data for the reaction 2 H2 (g) + Cl2 (g) are given in the table. What is the rate law for this reaction? (A) rate k [Cl2]2 (B) rate = k [Cl2] (C) rate = k [H2] (D) rate = k [H2] [Cl2]
A kinetic study of the reaction 2 ClO2(aq) + 2 OH -(aq) → ClO2- (aq) + ClO3- (aq) +   H2O(l) yielded the data shown on the image. A.  What is the rate of appearance of the ClO3- in experiment 1 (Be sure to inlcude units in this and other answers.)   B. Determine the experimental rate law.   C. Determine the value of the rate constant  based on your answer to Part C. (Inlude units)
If the rate for the following reaction is found to be the following: Rate = k [Cl2]3/2 • [HCCl3]. What are the units for the rate constant, k? Cl2 (g) + HCCl3 (g)       →      HCl (g) + CCl 4 (g)    
A reaction is second order in [A]. What happens to the rate when the concentration of A is doubled? A. The rate remains unchanged B. The rate increases by a factor of two C. The rate increases by a factor of three D. The rate increases by a factor of four E. The rate increases by a factor of nine
Given k = 7.8 x 10  - 2 s -1 for a reaction which is first order in A, what is the initial rate of the reaction (M/s) when the initial concentration of A is 0.0030 M? A. 2.3 x 10 -4 B. 7.9 x 10 -4 C. 9.2 x 10 -4 D. 2.6 x 101 E. 7.7 x 101
Initial rate data have been determined at a certain temperature for the gaseous reaction. The numerical value of the rate constant is: A. 7.5 B. 3.0 x 10 -3 C. 380 D. 0.75 E. 3.0 x 10 -4
The initial rate of a reaction which is first order in A is 1.0 × 10  −6 M/s when the initial concentration is 0.0040 M. What is the first order rate constant (s−1)? A. 4.0 × 10 -9 B. 1.0 × 10 -9 C. 2.5 × 10 -3 D. 1.0 × 10 -4 E. 2.5 × 10 -4
A first order reaction has a rate constant equal to 75 days -1. What is the rate constant in hrs-1?
The reaction A → B + C is known to be zero order in A with a rate constant of 3.0 × 10−2 mol/Ls at 25 °C. An experiment was run at 25 °C where [A] o = 1.0 × 10 -3 M. After 5.0 minutes the rate is? A. 5.0 × 10 -2mol/Ls B. 2.5 × 10 -2mol/Ls C. 1.25 × 10 -2mol/Ls D. 1.0 × 10 -3mol/Ls E. none of these
The reaction A + 2B → products has the rate law, rate = k [A][B]3. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase? A) 2 B) 4 C) 6 D) 8 E) 9
For the reaction: 2N2O5(g) → 4NO2(g) + O2(g) the rate constant is k = 2.8×10−3 sec−1. What is the order of the reaction? a) Second b) Zeroth c) Third d) First e) None of the above
The rate law of a reaction is rate = k[D][X]. What are the units of the rate constant? A. mol L-1s-1 B. L mol-1s-1 C. mol2 L-2s-1 D. mol L-1s-2 E. L2 mol -2s-1
The rate law for the reaction: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) is rate = k [Cl2]1/2[CHCl3]3/4. The units for the rate constant are a) M−1/4 sec−1 b) M1/4 sec−1 c) M−5/4 sec−1 d) M−1/2 sec−1 e) M−1 sec-1
A reaction was found to be second order in carbon monoxide concentration. If the concentration of carbon monoxide is tripled, the rate of the reaction a) remains unchanged b) doubles c) triples d) increases by a factor of 9 e) increases by a factor of 4
The following chemical reaction produced this chemical kinetics data. 
What is the overall order of the following reaction, given the rate law? 2NO (g) + H2 (g) ⇌ N2 (g) + 2H2O(g)  Rate = k [NO]2[H2]   A. 3rd order B. 0th order C. 1st order D. 2nd order E. 4th order
Based on your knowledge of rate law determine the answer. 
Based on your knowledge of rate law answer the following question. 
Determine the rate constant for the reaction between SO 2, O2, and H2O from the information given in the table below. a) 6.19x10−3 b) 1.37x10−2 c) 4.12x10−2 d) 3.09x10−4 e) 2.06x10−3    
For a certain reaction, the rate law is Rate = k[A][B] 1/2. What are the units of the rate constant? a) conc−3/2 s−1 b) conc−1/2 s c) conc s−1/2 d) conc1/2 s−1 e) conc−1/2 s−1
If the rate law for a reaction is given by Rate = k[A] 1/2[B]3 what will be the effect on the reaction rate if the concentration of A is increased by a factor of 4 and the concentration of B is lowered by a factor of 2?   a) Increase by a factor of 2 b) Remain unchanged c) Decrease by a factor of 4 d) Decrease by a factor of 21/2 e) Increase by a factor of 4
Determine the rate law for the reaction between I 2 and C3H7Br from the information given in the table below.  a) k[I2]1/2[C3H7Br] b) k[I2]1/2[C3H7Br]2 c) k[I2]1/3[C3H7Br]2 d) k[I2]1/4[ C3H7Br]2 e) k[I2]1/3[C3H7Br]  
The following table shows a series of experiements that were performed to determine the rate of NO2 production from O2 and NO: O2(g) + 2NO(g) → 2NO2(g)    a) What is the order with respect to O 2?        b) What is the order of the reaction with respect to NO?       c) What is the overall order of the reaction?  
For the reaction of chlorine and nitric oxide,  2NO(g) + Cl2(g) → 2NOCl(g) doubling the concentration of chlorine doubles the rate of reaction. Doubling the concentration of both reactants increases the rate of reaction by a factor of eight. The reaction is (A) first order in both NO and Cl 2. (B) first order in NO and second order in Cl 2. (C) second order in NO and first order in Cl 2. (D) second order in both NO and Cl 2.
A plot of 1/concentration of A (M-1) vs time (min) gave a straight line with the following formula: y = 0.20x + 2.0. Which of the following is the correct expression for the rate law? Assume a =1. a) Rate = 0.2 M-1 min-1 b) Rate = 0.2 M-1 min-1 [A] c) Rate = -0.2 M-1 min-1 [A] d) Rate = 0.2 M-1 min-1 [A]2 e) Rate = -0.2 M-1 min-1 [A]2
Many gaseous reactions occur in a car engine and exhaust system. One of these is represented by the following equation: NO2 (g) + CO (g) ⇄ NO (g) + CO2 (g) What is the rate of the reaction if the concentrations of NO2 and CO are 0.25 M and 0.30 M respectively?  For the choices below, what is the order of reaction for NO2?
The reaction below has an initial rate of 0.070 M/s. What will the initial rate be if [A] is halved and [B] is tripled?  A  +  B  →  C  +  D         Rate = k [A][B]  2 a) 0.105 M/s b) 0.000343 M/s c) 0.315 M/s d) 0.210 M/s e) 0.0098 M/s
Using the given data, determine the rate constant of this reaction. A + 2 B → C + D Given Data: Trial       [A](M)     [B](M)       RATE (M/s) 1            0.310      0.340          0.0213 2            0.310      0.680          0.0213 3            0.620      0.340          0.0852  
The reaction between acetone and bromine in acid solution is represented by the equation CH3OCH3(aq) + Br2(aq) + H3O+(aq) → products The tabulated kinetic data were gathered. Based on these data, the experimental rate law is:
A certain chemical reaction has the following rate law Rate = k [A]2[B]3[C]-2[D] What are the units of the rate constant for this reaction? 
If the rate law for the following reaction is found to be the following: Rate = [Cl2]3/2 • [HCCl3].  What are the units for the rate constant, k?  Cl2 (g) + HCCl3 → (g) HCl (g)  +   CCl4 (g)  
Given the initial concentrations in  Kinetics Data Table 1, predict what the rate would be if the initial concentrations were [A] = 0.062 M, [B] = 1.03 M, and [C] = 1.12 M. 2 A + 3 B + C → 2 D + E a. 2.026 M/s b. 0.126 M/s c. 2.086 M/s d. 1.863 M/s e. 0.112 M/s  
Cyclopentadiene (C5H6) reacts with itself to form dicyclopentadiene (C10H12). A 0.0400 M solution of C5H6 was monitored as a function of time as the reaction 2C5H6 C10H12 proceeded. The following data were collected: Time (s) [C5H6] (M) 0.0 0.0400 50.0 0.0300 100.0 0.0240 150.0 0.0200 200.0 0.0174 Plot 1/[C5H6] versus time.
The graph below shows a plot of the rate of a reaction versus the concentration of the reactant A for the reaction A .What is the order of the reaction with respect to A?
The graph below shows a plot of the rate of a reaction versus the concentration of the reactant A for the reaction A .Write a rate law for the reaction.
How is the order of a reaction generally determined?
For a reaction with multiple reactants (Rate = k [A]m[B]n), how is the overall order of the reaction defined?
A colored dye compound decomposes to give a colorless product. The original dye absorbs at 608 nm and has an extinction coefficient of 4.7 104 M-1 cm-1 at that wavelength. You perform the decomposition reaction in a 1-cm cuvette in a spectrometer and obtain the following data: Time (min) Absorbance at 608 nm 0 1.254 30 0.941 60 0.752 90 0.672 120 0.545 From these data, determine the rate law for the reaction "dye ightarrow product".
A reaction A + B obeys the following rate law: Rate = k [B]2.What is the reaction order for B?
A reaction A + B obeys the following rate law: Rate = k [B]2.What is the overall reaction order?
The graph below shows a plot of the rate of a reaction versus the concentration of the reactant .What is the order of the reaction with respect to A?
The graph below shows a plot of the rate of a reaction versus the concentration of the reactant .Write a rate law for the reaction.
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.Write a rate law for the reaction.
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.What is the overall order of the reaction?
Cyclopentadiene (C5H6) reacts with itself to form dicyclopentadiene (C10H12). A 0.0400 M solution of C5H6 was monitored as a function of time as the reaction 2C5H6 C10H12 proceeded. The following data were collected: Time (s) [C5H6] (M) 0.0 0.0400 50.0 0.0300 100.0 0.0240 150.0 0.0200 200.0 0.0174 What is the value of the rate constant?
A reaction A + B obeys the following rate law: Rate = k [B]2.Will the rate constant change?
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.By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)?
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.By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?
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.By what factor does the reaction rate change if the concentrations of all three reactants are doubled?
A reaction A + B obeys the following rate law: Rate = k [B]2.If [A] is doubled, how will the rate change?
A student says, “The initial concentration of a reactant was doubled, and the rate doubled. Therefore the reaction is second order in that reactant.” Why might the student say that? What is wrong with the statement? What is the actual order with respect to the reactant?
Consider a reaction with the following rate law. Rate = k [X]2[Y]3[Z]-1 What are the units of the rate constant for this reaction? A. M-4 time-1 B. M-3 time-1 C. M time -1 D. M4 time-1 E. M3 time-1
Consider this initial-rate data at a certain temperature for the reaction described by 2NO2(g) + O3(g) → N2O5 (g) +O2 (g) Determine the value and units of the rate constant.
Consider this initial-rate data at a certain temperature for the reaction described by:   N2O3(g) → NO(g) + NO2(g) Determine the value and units of the rate constant.  
Write the rate law for these two elementary reaction equations.(a) 2A(g) + B(g) → C(g) + D(g)(b) X(R) + Y(g) → Z(g) 
Consider the following elementary reaction equation. 2O2(g) + Cl(g) → ClO(g) + O3(g) a) What is the order with respect to O 2. b) What is the overall order of the reaction. c) Classify the reaction as a unimolecular, bimolecular, or termolecular.
For the following rate law rate = k[A]x. Determine the value of x if:a) the rate doubles when [A] is doubled.b) no change in rate occurs when [A] is doubled.
CH3Br + NaOH ->CH3OH + NaBrWhen the concentration of CH3Br and NaOH are both 0.100M, the rate of the reaction is 0.0050 M/s. a. What is the rate of the reaction if the concentration of CH3Br is doubled? _____M/s b. What is the rate of the reaction if the concentration of NaOH is halved? _____M/s c. What is the rate of the reaction if the concentrations of CH3Br and NaOH are both increased by a factor of six? ____M/s
Consider the reaction described by the following equation.C2H4Br2(aq) + 3I- (aq) → C2H4(g)+2Br- (aq)+I3-(aq)The rate law israte = k[C2H4Br2] [I-]     where k= 4.91 x 10-3 M-1 • s-1What are the missing entries in the following table?  
Consider this reaction and its rate law. 3A + 2B → products rate = k[A][B] a) What is the order with respect to A? b) What is the order with respect to B? c) What is the overall reaction order?
Consider the reaction 
For the reaction (CH3)3CBr(aq) + OH-(aq) → (CH3)3COH(aq) + Br-(aq), the following data were obtained at 55 °C. What is the rate constant? a) 1.0 x 10-4 s-1 b) 2.0 x 10-2 s-1 c) 2.0 x 10-3 s-1 d) 1.0 x 10-2 s-1 e) 1.0 x 10-1 s-1
You and a coworker have developed a molecule that has shown potential as cobra antivenin (AV). This antivenin works by binding to the venom (V), thereby rendering it nontoxic. This reaction can be described by the rate lawRate = k[AV]1 [V]1You have been given the following data from your coworker:[V]0 = 0.20 M[AV]0 = 1.0 x 10 -4 MA plot of ln[AV] versus t (s) gives a straight line with a slope of -0.32 s  -1. What is the value of the rate constant (k) for this reaction?
The following reaction is a single-step, bimolecular reaction:CH3Br+NaOH → CH3OH+NaBr.When the concentrations of CH3Br and NaOH are both 0.170 M, the rate of the reaction is 0.0090 M/s.a. What is the rate of the reaction if the concentration of CH3Br is doubled?b. What is the rate of the reaction if the concentration of NaOH is halved?c. What is the rate of the reaction if the concentrations of CH3Br and NaOH are both increased by a factor of five? 
For the reaction A(g) + 2B(g) → 2C(g) + 2D(g), the following data was collected at constant temperature. Determine the correct rate law for this reaction. a) Rate = k[A][B] b) Rate = k[A]2[B] c) Rate = k[A][B]2 d) Rate = k[A] e) Rate = k[A]3
What are dimensions of rate constant units for third-order reaction, give an example.
Fill in the units for the apparent rate constant for each reaction order given below.
For the reaction A +B+ C → D + E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected:What is the value of the rate constant k for this reaction? Express your answer to two significant figures and include the appropriate units.  
Calculate the initial rate for the formation of C at 25°C, if [A]=0.50M and [B]=0.075M. Express your answer to two significant figures and include the appropriate units. Consider the reactionA+2B → Cwhose rate at 25°C was measured using three different sets of initial concentrations as listed in the following table: Trial                    [A]                    [B]                    Rate                          (M)                   (M)                    (M/s)1                       0.20                 0.030                1.4 x 10 - 3  2                       0.20                 0.060                2.9 x 10      - 33                       0.40                 0.030                5.8 x 10       - 3  
The reaction A + B → C + D             rate = k[A][B]  2 has an initial rate of 0.0110 M/s. What will the initial rate be if [A] is halved and [B] is tripled? _____ M/s What will the initial rate be if [A] is tripled and [B] is halved? _____ M/s
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide describe by:O3(g) + NO(g) → O2(g) + NO2(g)The rate law for this reaction is:rate of reaction = k[O3][NO]a. Given that k = 3.66x10 6 M-1 s-1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O 3]0 = 2.25x10-6 M and [NO]0 = 4.37x10-5 M, owing to continuous production from separate sources. (M s-1)b. Calculate the number of moles of NO2(g) produced per hour per liter of air. (mol h -1  L-1) 
Using the given data, calculate the rate constant of this reaction.                                     A+B →  C+DTrial            [A](M)          [B](M)          Rate(M/s)                   k=_____?1                  0.340           0.200           0.0142                 2                  0.340           0.520           0.0960                 3                  0.476           0.200           0.0199                                     
The following reaction is a single-step, bimolecular reaction:CH3Br +NaOH → CH3OH +NaBrWhen the concentrations of CH3Br and NaOH are both 0.125 M, the rate of the reaction is 0.0060 M/sa. What is the rate of the reaction if the concentration of CH3Br is doubled?b. What is the rate of the reaction if the concentration of NaOH is halved?c. What is the rate of the reaction if the concentration of CH3Br and NaOH are both increased by a factor of six?
Consider the following data showing the initial rate of a reaction (A → products) at several different concentrations of A.What is the order of the reaction?[A]  (M)Initial Rate (M/s)0.1000.0650.2000.1300.3000.195
Experiments were conducted to study the rate of the reaction represented by this equation.[2] 2 NO(g) + 2 H2(g) ⟶ N2(g) + 2 H2O(g) Initial concentrations and rates of reaction are given here.Consider the following questions: (a) Determine the order for each of the reactants, NO and H2, from the data given and show your reasoning.
Consider the following general reaction and data:2A + 2B + C ⟶ D + 3E(a) What is the reaction order with respect to each reactant?
Consider the following data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A]  (M)Initial Rate (M/s)0.1000.0650.2000.1300.3000.195Write a rate law for the reaction.
Experiments were conducted to study the rate of the reaction represented by this equation.[2] 2 NO(g) + 2 H2(g) ⟶ N2(g) + 2 H2O(g) Initial concentrations and rates of reaction are given here.Consider the following questions:(b) Write the overall rate law for the reaction.
Consider the following data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A] (M) Initial rate (M/s)0.150.0090.300.0190.600.038What is the order of the reaction?
Consider the following data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A] (M) Initial rate (M/s)0.150.0090.300.0190.600.038Specify a rate law for the reaction.
Consider the following general reaction and data:2A + 2B + C ⟶ D + 3E(c) Write the rate law for this reaction.
The data below were collected for the following reaction: 2NO2(g) + F2(g) → 2 NO2F(g) [NO2] (M)  [F2] (M)  Initial Rate (M/s) 0.1000.1000.0260.2000.1000.0510.2000.2000.1030.4000.4000.411What is the overall order of the reaction?
The data below were collected for the following reaction: 2NO2(g) + F2(g) → 2 NO2F(g) [NO2] (M)  [F2] (M)  Initial Rate (M/s) 0.1000.1000.0260.2000.1000.0510.2000.2000.1030.4000.4000.411Write an expression for the reaction rate law.
The data below were collected for the following reaction: CH3Cl(g) + 3Cl2(g) → CCl4(g) + 3HCl(g)[CH3Cl] (M)[Cl2] (M)Initial Rate (M/s)0.0500.0500.0140.1000.0500.0290.1000.1000.0410.2000.2000.115Write an expression for the reaction rate law.
The data below were collected for the following reaction: CH3Cl(g) + 3Cl2(g) → CCl4(g) + 3HCl(g)[CH3Cl] (M)[Cl2] (M)Initial Rate (M/s)0.0500.0500.0140.1000.0500.0290.1000.1000.0410.2000.2000.115What is the overall order of the reaction?
BF3 (g) + NH3(g) → F3BNH3 (g)For the above reaction, the following data were measured:Experiment [BF3]  (M)  [NH3]  (M) Initial Rate (M/s) 10.2500.2500.213020.2500.1250.106530.2000.1000.068240.3500.1000.119350.1750.1000.0596What is the rate law for the reaction?
The citric acid cycle is the central reaction sequence in the cellular metabolism of humans and many other organisms. One of the key steps is catalyzed by the enzyme isocitrate dehydrogenase and the oxidizing agent NAD+. In yeast, the reaction is eleventh order:Rate = k[enzyme] [isocitrate]4 [AMP]2 [NAD+]m [Mg2+]2What is the order with respect to NAD+?
The reaction2NO (g) + Cl2 (g) → 2NOCl (g)was studied at -10°C. The following results were obtained whereRate = -Δ[Cl2] / Δta. What is the rate law? 
The decomposition of nitrosyl chloride was studied:2NOCl (g) ⇌ 2NO (g) + Cl2 (g)The following data were obtained wherea. What is the rate law? 
The rate of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20°C. The following data were collected with all concentration units in μmol/L. (A hemoglobin concentration of 2.21 μmol/L is equal to 2.21 x 10-6 mol/L.)b. Determine the rate law. 
The reactionI - (aq) + OCl - (aq) → IO - (aq) + Cl - (aq)was studied, and the following data were obtained:a. What is the rate law? 
The rate of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20°C. The following data were collected with all concentration units in μmol/L. (A hemoglobin concentration of 2.21 μmol/L is equal to 2.21 x 10-6 mol/L.)a. Determine the orders of this reaction with respect to Hb and CO. 
The following reaction was monitored as a function of time: A → B + C. A plot of ln[A] versus time yields a straight line with slope −4.4×10−3 /s. Write the rate law for the reaction.
The gas-phase decomposition of NO2, NO2 (g) → 2 NO (g) + O2 (g), is studied at 383 oC, giving the following data:Time (s)[NO2] (M)0.00.1005.00.01710.00.009015.00.006220.00.0047Is the reaction first order or second order with respect to the concentration of NO2?
Carbon disulfide, a poisonous, flammable liquid, is an excellent solvent for phosphorus, sulfur, and some other nonmetals. A kinetic study of its gaseous decomposition gave these data:Write the rate law for the decomposition of CS 2.
What is the order of reaction with respect to A and B for a reaction that obeys the rate law rate = k[A]2[B]3?
In a clock reaction, a dramatic color change occurs at a time determined by concentration and temperature. Consider the iodine clock reaction, whose overall equation is2 I−(aq) + S 2O82−(aq) ⟶ I 2(aq)