Deck 14: Chemical Kinetics

Question 1

Determine the rate law and the value of k for the following reaction using the data provided. 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

Answer 1

Rate = 11 M^-3/2s^-1 [CO][Cl₂]^3/2

Question 2

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]⁰[B]²,what is the new rate if the concentration of [A] is increased to 0.200 M?

A) 0.0200 M/s
B) 0.0400 M/s
C) 0.0600 M/s
D) 0.0800 M/s
E) 0.100 M/s

Answer 2

0.0200 M/s

Question 3

Give the characteristic of a second-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.

Answer 3

The rate of the reaction is proportional to the square of the concentration of the reactant.

Question 4

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.

Question 5

Give the characteristic of a zero-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.

Question 6

A gas chromatograph can be used to determine the relative amounts of reactants and products by

A) measuring the changes in pressure as the reaction proceeds.
B) analyzing the intensity of the transmitted light.
C) separating the components of the mixture, which results in an individual peak for each component and the peaks are quantified.
D) measuring the degree of the polarization of light.
E) measuring the change in temperature of the reaction.

Question 7

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]¹,what is the new rate if the concentration of [A] is increased to 0.200 M?

A) 0.0200 M/s
B) 0.0400 M/s
C) 0.0600 M/s
D) 0.0800 M/s
E) 0.100 M/s

Question 8

What is the overall order of the following reaction,given the rate law? NO(g)+ O₃(g)→ NO₂(g)+ O₂(g)Rate = k[NO][O₃]

A) 1st order
B) 2nd order
C) 3rd order
D) 1 order
E) 0th order

Question 9

Identify the CFC with the longest atmospheric lifetime.

A) CFC-113
B) CFC-12
C) CFC-114
D) CFC-11
E) CFC-115

Question 10

Write a balanced reaction for which the following rate relationships are true. Rate = = = -

A) N₂ + O₂ →

N₂O
B) 2 N₂O → 2 N₂ + O₂
C) N₂O → N₂ + 2 O₂
D) N₂O →
N₂ + O₂
E) 2 N₂ + O₂ → 2 N₂O

Question 11

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]⁰,what is the new rate if the concentration of [A] is increased to 0.200 M?

A) 0.0200 M/s
B) 0.0400 M/s
C) 0.0600 M/s
D) 0.0800 M/s
E) 0.100 M/s

Question 12

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]²,what is the new rate if the concentration of [A] is increased to 0.200 M?

A) 0.0200 M/s
B) 0.0400 M/s
C) 0.0600 M/s
D) 0.0800 M/s
E) 0.100 M/s

Question 13

Determine the rate law and the value of k for the following reaction using the data provided. NO₂(g)+ O₃(g)→ NO₃(g)+ O₂(g)[NO₂]_i (M)[O₃]_i (M)Initial Rate (M^-1s^-1)
0)10 0.33 1.42
0)10 0.66 2.84
0)25 0.66 7.10

A) Rate = 1360 M^-2.5s^-1[NO₂]^2.5[O₃]
B) Rate = 227 M^-2.5s^-1[NO₂][O₃]^2.5
C) Rate = 43 M^-1s^-1[NO₂][O₃]
D) Rate = 430 M^-2s^-1[NO₂]²[O₃]
E) Rate = 130 M^-2s^-1[NO₂][O₃]²

Question 14

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g)+ O₂(g)→ 2 NO₂(g)[NO]_i (M)[O₂]_i (M)Initial Rate (M^-1s^-1)
0)030 0.0055 8.55 × 10^-3
0)030 0.0110 1.71 × 10^-2
0)060 0.0055 3.42 × 10^-2

A) Rate = 57 M^-1s^-1[NO][O₂]
B) Rate = 3.8 M^-1/2s^-1[NO][O₂]^1/2
C) Rate = 3.1 × 10⁵ M^-3s^-1[NO]²[O₂]²
D) Rate = 1.7 × 10³ M^-2s^-1[NO]²[O₂]
E) Rate = 9.4 × 10³ M^-2s^-1[NO][O₂]²

Question 15

Identify the CFC with the shortest atmospheric lifetime.

A) CFC-113
B) CFC-12
C) CFC-114
D) CFC-11
E) CFC-115

Question 16

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A][B]²,what is the new rate if the concentration of [A] is increased to 0.200 M?

A) 0.0200 M/s
B) 0.0400 M/s
C) 0.0600 M/s
D) 0.0800 M/s
E) 0.100 M/s

Question 17

Write a balanced reaction for which the following rate relationships are true. Rate = - = =

A) 2 N₂O₅ → 4 NO₂ + O₂
B) 4 NO₂ + O₂ → 2 N₂O₅
C) 2 N₂O₅ → NO₂ + 4 O₂
D) NO₂ + O₂ →

N₂O₅
E) N₂O₅ →

NO₂ + O₂

Question 18

Identify the methods used to monitor a reaction as it occurs in the reaction flask.

A) polarimeter
B) spectrometer
C) pressure measurement
D) none of the above
E) all of the above

Question 19

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]²[B]²,what is the new rate if the concentration of [A] is increased to 0.200 M?

A) 0.0200 M/s
B) 0.0400 M/s
C) 0.0600 M/s
D) 0.0800 M/s
E) 0.100 M/s

Question 20

Determine the rate law and the value of k for the following reaction using the data provided. S₂O₈²⁻(aq)+ 3 I⁻(aq)→ 2 SO₄²⁻(g)+ I₃⁻(aq)[S₂O₈²⁻]_i (M)[I⁻]_i (M)Initial Rate (M^-1s^-1)
0)30 0.42 4.54
0)44 0.42 6.65
0)44 0.21 3.33

A) Rate = 120 M^-2s^-1 [S₂O₈^2⁻]²[I⁻]
B) Rate = 36 M^-1s^-1 [S₂O₈²⁻][I⁻]
C) Rate = 86 M^-2s^-1 [S₂O₈²⁻][I⁻]²
D) Rate = 195 M^-3s^-1 [S₂O₈²⁻]²[I⁻]²
E) Rate = 23 M^-1/2s^-1 [S₂O₈²⁻][I⁻]^1/2

Question 21

The second-order decomposition of HI has a rate constant of 1.80 × 10^-3 M^-1s^-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

A) 4.55 M
B) 0.258 M
C) 3.87 M
D) 2.20 M
E) 2.39 M

Question 22

The first-order decomposition of N₂O₅ at 328 K has a rate constant of 1.70 × 10^-3 s^-1.If the initial concentration of N₂O₅ is 2.88 M,what is the concentration of N₂O₅ after 12.5 minutes?

A) 0.124 M
B) 0.805 M
C) 2.82 M
D) 0.355 M
E) 0.174 M

Question 23

The first-order decomposition of N₂O at 1000 K has a rate constant of 0.76 s^-1.If the initial concentration of N₂O is 10.9 M,what is the concentration of N₂O after 9.6 s?

A) 7.4 × 10^-3 M
B) 1.0 × 10^-3 M
C) 1.4 × 10^-3 M
D) 3.6 × 10^-3 M
E) 8.7 × 10^-3 M

Question 24

What data should be plotted to show that experimental concentration data fits a second-order reaction?

A) ln[reactant] vs. time
B) [reactant] vs. time
C) ln(k) vs. 1/T
D) 1/[reactant] vs. time
E) ln(k) vs. E_a

Question 25

The second-order decomposition of NO₂ has a rate constant of 0.255 M^-1s^-1.How much NO₂ decomposes in 4.00 s if the initial concentration of NO₂ (1.00 L volume)is 1.33 M?

A) 1.8 mol
B) 0.85 mol
C) 0.48 mol
D) 0.77 mol
E) 0.56 mol

Question 26

The rate constant for the first-order decomposition of N₂O is 3.40 s^-1.What is the half-life of the decomposition?

A) 0.491 s
B) 0.204 s
C) 0.236 s
D) 0.424 s
E) 0.294 s

Question 27

Which of the following statements is FALSE?

A) The average rate of a reaction decreases during a reaction.
B) It is not possible to determine the rate of a reaction from its balanced equation.
C) The rate of zero-order reactions is not dependent on concentration.
D) The half-life of a first-order reaction is dependent on the initial concentration of reactant.
E) None of the statements is FALSE.

Question 28

What data should be plotted to show that experimental concentration data fits a first-order reaction?

A) 1/[reactant] vs. time
B) [reactant] vs. time
C) ln[reactant] vs. time
D) ln(k) vs. 1/T
E) ln(k) vs. E_a

Question 29

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10^-4 s^-1.If the initial concentration of cyclopropane is 1.33 M,what is the concentration of cyclopropane after 644 s?

A) 0.43 M
B) 0.15 M
C) 0.94 M
D) 0.86 M
E) 0.67 M

Question 30

Identify the rate-determining step.

A) the slowest step
B) the faster step
C) the fast step
D) always the last step
E) always the second step

Question 31

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 M.What is the rate constant for this reaction?

A) 1.0 × 10^-2 M^-1s^-1
B) 4.5 × 10^-2 M^-1s^-1
C) 9.7 × 10^-2 M^-1s^-1
D) 2.2 × 10^-2 M^-1s^-1
E) 3.8 × 10^-2 M^-1s^-1

Question 32

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon decompose after 5.55 days if the sample initially weighs 100.0 grams?

A) 83.4 g
B) 16.6 g
C) 50.0 g
D) 36.6 g
E) 63.4 g

Question 33

Which of the following statements is FALSE?

A) The half-life of a zero-order reaction is dependent on concentration.
B) The half-life of a second-order reaction is not dependent on concentration.
C) The rate of second-order reactions is dependent on concentration.
D) The rate of a first-order reaction is dependent on concentration.
E) None of the statements is FALSE.

Question 34

The first-order rearrangement of CH₃NC is measured to have a rate constant of 3.61 × 10^-15 s^-1 at 298 K and a rate constant of 8.66 × 10^-7 s^-1 at 425 K.Determine the activation energy for this reaction.

A) 160. kJ/mol
B) 240. kJ/mol
C) 417 kJ/mol
D) 127 kJ/mol
E) 338 kJ/mol

Question 35

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon remain after 7.22 days if the sample initially weighs 250.0 grams?

A) 4.21 g
B) 183 g
C) 54.8 g
D) 76.3 g
E) 67.5 g

Question 36

Carbon-14 has a half-life of 5720 years and this is a first-order reaction.If a piece of wood has converted 75% of the carbon-14,then how old is it?

A) 11440 years
B) 2375 years
C) 4750 years
D) 4290 years
E) 1430 years

Question 37

What data should be plotted to show that experimental concentration data fits a zeroth-order reaction?

A) ln[reactant] vs. time
B) 1/[reactant] vs. time
C) ln(k) vs. 1/T
D) ln(k) vs. E_a
E) [reactant] vs. time

Question 38

Carbon-14 has a half-life of 5720 years and this is a first-order reaction.If a piece of wood has converted 25% of the carbon-14,then how old is it?

A) 11440 years
B) 2375 years
C) 4750 years
D) 4290 years
E) 1430 years

Question 39

The half-life for the decay of radium is 1620 years.What is the rate constant for this first-order process?

A) 4.28 × 10^-4 yr^-1
B) 1.12 × 10^-4 yr^-1
C) 2.33 × 10^-4 yr^-1
D) 8.91 × 10^-4 yr^-1
E) 6.17 × 10^-4 yr^-1

Question 40

For a reaction,what generally happens if the temperature is increased?

A) A decrease in k occurs, which results in a faster rate.
B) A decrease in k occurs, which results in a slower rate.
C) An increase in k occurs, which results in a faster rate.
D) An increase in k occurs, which results in a slower rate.
E) There is no change with k or the rate.

Question 41

Given the following balanced equation,determine the rate of reaction with respect to [O₂]. 2 SO₂(g)+ O₂(g)→ 2 SO₃(g)

A) Rate = -

B) Rate = +

C) Rate = -
D) Rate = -
E) It is not possible to determine without more information.

Question 42

Identify an heterogeneous catalyst.

A) CFCs with ozone
B) Pd in H₂ gas
C) KI dissolved in H₂O₂
D) H₂SO₄ with concentrated HCl
E) H₃PO₄ with an alcohol

Question 43

If the activation energy for a given compound is found to be 42.0 kJ/mol,with a frequency factor of 8.0 × 10¹⁰ s^-1,what is the rate constant for this reaction at 298 K?

A) 2.9 × 10^-4 s^-1
B) 7.4 × 10^-4 s^-1
C) 1.4 × 10⁹ s^-1
D) 4.6 × 10⁵ s^-1
E) 3.5 × 10³ s^-1

Question 44

Which rate law has a molecularity of three?

A) Rate = k[A]⁰
B) Rate = k[A][B]²
C) Rate = k[A][B]
D) Rate = k[A]
E) Rate = k[A]²

Question 45

Biological catalysts that increase the rates of biochemical reactions are known as

A) substrates.
B) inhibitors.
C) enzymes.
D) binders.
E) trumanettes.

Question 46

If the activation energy for a given compound is found to be 103 kJ/mol,with a frequency factor of 4.0 × 10¹³ s^-1,what is the rate constant for this reaction at 398 K?

A) 1.2 s^-1
B) 8.2 s^-1
C) 3.9 × 10¹⁰ s^-1
D) 1.7 × 10¹⁰ s^-1
E) 2.5 × 10⁷ s^-1

Question 47

In the hydrogenation of double bonds,a catalyst is needed.In the third step,the reactants react to form the product.This step is known as

A) adsorption.
B) diffusion.
C) reaction.
D) desorption.
E) none of the above

Question 48

A reaction is followed and found to have a rate constant of 3.36 × 10⁴ M^-1s^-1 at 344 K and a rate constant of 7.69 M^-1s^-1 at 219 K.Determine the activation energy for this reaction.

A) 23.8 kJ/mol
B) 42.0 kJ/mol
C) 11.5 kJ/mol
D) 12.5 kJ/mol
E) 58.2 kJ/mol

Question 49

In the hydrogenation of double bonds,a catalyst is needed.In the first step,the reactants must come into contact with a metal surface.This step is known as

A) adsorption.
B) diffusion.
C) reaction.
D) desorption.
E) none of the above

Question 50

Which rate law has a molecularity of one?

A) Rate = k[A]⁰
B) Rate = k[A][B]
C) Rate = k[A][B][C]
D) Rate = k[A]
E) Rate = k[A]²

Question 51

In the hydrogenation of double bonds,a catalyst is needed.In the second step,the reactants diffuse on the surface until they approach each other.This step is known as

A) adsorption.
B) diffusion.
C) reaction.
D) desorption.
E) none of the above

Question 52

In the hydrogenation of double bonds,a catalyst is needed.In the last step,the reactants must escape from the surface into the gas phase.This step is known as

A) adsorption.
B) diffusion.
C) reaction.
D) desorption.
E) none of the above

Question 53

Given the following balanced equation,determine the rate of reaction with respect to [SO₂]. 2 SO₂(g)+ O₂(g)→ 2 SO₃(g)

A) Rate = -

B) Rate =

C) Rate = +
D) Rate = -
E) It is not possible to determine without more information.

Question 54

A reaction is found to have an activation energy of 108 kJ/mol.If the rate constant for this reaction is 4.60 × 10^-6 s^-1 at 275 K,what is the rate constant at 366 K?

A) 12 s^-1
B) 1.7 s^-1
C) 0.58 s^-1
D) 5.4 × 10^-5 s^-1
E) 1.9 × 10^-4 s^-1

Question 55

Given the following balanced equation,determine the rate of reaction with respect to [SO₃]. 2 SO₂(g)+ O₂(g)→ 2 SO₃(g)

A) Rate = -

B) Rate = +

C) Rate = +
D) Rate = -
E) It is not possible to determine without more information.

Question 56

Which of the following statements is TRUE?

A) The rate constant does not depend on the activation energy for a reaction where the products are lower in energy than the reactants.
B) A catalyst raises the activation energy of a reaction.
C) Rate constants are temperature dependent.
D) The addition of a homogeneous catalyst does not change the activation energy of a given reaction.
E) None of the above is true.

Question 57

Which rate law has a molecularity of three?

A) Rate = k[A]⁰
B) Rate = k[A][B]
C) Rate = k[A][B][C]
D) Rate = k[A]
E) Rate = k[A]²

Question 58

Which rate law is unimolecular?

A) Rate = k[A]²
B) Rate = k[A][B]
C) Rate = k[A][B][C]
D) Rate = k[A]
E) Rate = k[A]3

Question 59

Which rate law has a molecularity of two?

A) Rate = k[A]⁰
B) Rate = k[A][B]
C) Rate = k[A][B][C]
D) Rate = k[A]
E) Rate = k[A]³

Question 60

A reaction is found to have an activation energy of 38.0 kJ/mol.If the rate constant for this reaction is 1.60 × 10² M^-1s^-1 at 249 K,what is the rate constant at 436 K?

A) 2.38 × 10⁵ M^-1s^-1
B) 1.26 × 10³ M^-1s^-1
C) 7.94 × 10⁴ M^-1s^-1
D) 4.20 × 10⁵ M^-1s^-1
E) 3.80 × 10⁴ M^-1s^-1

Question 61

What are the units of k in the following rate law? Rate = k[X] [Y]³

A)
B)
C) M s²
D)
E)

Question 62

What are the units of k in a zero-order reaction?

A)
B) M
C)
D)
E)

Question 63

The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)
If the rate of appearance of O₂ is equal to 3.00 mol/min at a particular moment,what is the rate of disappearance of N₂O₅ at that moment?

A) 0.750 mol/min
B) 1.50 mol/min
C) 6.00 mol/min
D) 12.0 mol/min

Question 64

What are the units of k in a second-order reaction?

A)
B) M²s²
C)
D)
E)

Question 65

The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)
If the rate of disappearance of N₂O₅ is equal to 1.80 mol/min at a particular moment,what is the rate of appearance of NO₂ at that moment?

A) 0.900 mol/min
B) 1.80 mol/min
C) 3.60 mol/min
D) 7.20 mol/min
E) 1.50 mol/min

Question 66

Given the following balanced equation,determine the rate of reaction with respect to [NOCl]. 2 NO(g)+ Cl₂(g)→ 2 NOCl(g)

A) Rate = -

B) Rate = +

C) Rate = -

D) Rate = -
E) It is not possible to determine without more information.

Question 67

Given the following balanced equation,determine the rate of reaction with respect to [O₂]. 2 O₃(g)→ 3 O₂(g)

A) Rate = +
B) Rate = -

C) Rate = +

D) Rate = +
E) It is not possible to determine without more information.

Question 68

Given the following balanced equation,determine the rate of reaction with respect to [Cl₂].If the rate of Cl₂ loss is 4.24 × 10^-2 M/s,what is the rate of formation of NOCl? 2 NO(g)+ Cl₂(g)→ 2 NOCl(g)

A) 4.24 × 10^-2 M/s
B) 2.12 × 10^-2 M/s
C) 1.06 × 10^-1 M/s
D) 8.48 × 10^-2 M/s
E) 1.61 × 10^-2 M/s

Question 69

What are the units of k in the following rate law? Rate = k[X]²[Y]

A)
B)
C) M²s²
D)
E)

Question 70

Given the following balanced equation,determine the rate of reaction with respect to [HCl]. H₂(g)+ Cl₂(g)→ 2 HCl(g)

A) Rate = +
B) Rate = -
C) Rate = -

D) Rate = +

E) It is not possible to determine without more information.

Question 71

Given the following balanced equation,determine the rate of reaction with respect to [O₂].If the rate of formation of O₂ is 7.78 × 10^-1 M/s,what is the rate of the loss of O₃? 2 O₃(g)→ 3 O₂(g)

A) 0.519 M/s
B) 1.56 M/s
C) 2.34 M/s
D) 1.17 M/s
E) 7.78 M/s

Question 72

What are the units of k in the following rate law? Rate = k[X][Y]

A)
B) M s²
C)
D)
E)

Question 73

Determine the rate law and the value of k for the following reaction using the data provided. 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)[N₂O₅]_i (M)Initial Rate (M^-1s^-1)
0)093 4.84 × 10^-4
0)084 4.37 × 10^-4
0)224 1.16 × 10^-3

A) Rate = 5.6 × 10^-2 M^-1s^-1[N₂O₅]²
B) Rate = 6.0 × 10^-1 M^-2s^-1[N₂O₅]³
C) Rate = 1.6 × 10^-3 M^1/2s^-1[N₂O₅]^1/2
D) Rate = 1.7 × 10^-2 M^-1/2s^-1[N₂O₅]^3/2
E) Rate = 5.2 × 10⁻³ s^-1[N₂O₅]

Question 74

Given the following balanced equation,determine the rate of reaction with respect to [H₂]. N₂(g)+ 3 H₂(g)→ 2 NH₃(g)

A) Rate = +
B) Rate = +

C) Rate = +

D) Rate = -

E) It is not possible to determine without more information.

Question 75

The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)
If the rate of appearance of NO₂ is equal to 0.560 mol/min at a particular moment,what is the rate of appearance of O₂ at that moment?

A) 0.140 mol/min
B) 0.280 mol/min
C) 1.12 mol/min
D) 2.24 mol/min

Question 76

Given the following balanced equation,determine the rate of reaction with respect to [NH₃]. N₂(g)+ 3 H₂(g)→ 2 NH₃(g)

A) Rate = +
B) Rate = -
C) Rate = +

D) Rate = -

E) It is not possible to determine without more information.

Question 77

Given the following balanced equation,determine the rate of reaction with respect to [O₂].If the rate of O₂ loss is 2.64 × 10^-3 M/s,what is the rate of formation of SO₃? 2 SO₂(g)+ O₂(g)→ 2 SO₃(g)

A) 2.64 × 10^-3 M/s
B) 1.19 × 10^-3 M/s
C) 1.32 × 10^-3 M/s
D) 6.60 × 10^-2 M/s
E) 5.28 × 10^-3 M/s

Question 78

Given the following balanced equation,determine the rate of reaction with respect to [Cl₂].If the rate of disappearance of Cl₂ is 4.24 × 10^-2 M/s,what is the rate of formation of NO? 2 NO(g)+ Cl₂(g)→ 2 NOCl(g)

A) 4.24 × 10^-2 M/s
B) 2.12 × 10^-2 M/s
C) 1.06 × 10^-1 M/s
D) 8.48 × 10^-2 M/s
E) 1.61 × 10^-2 M/s

Question 79

Given the following balanced equation,determine the rate of reaction with respect to [N₂]. N₂(g)+ 3 H₂(g)→ 2 NH₃(g)

A) Rate = +
B) Rate = -
C) Rate = +

D) Rate = -

E) It is not possible to determine without more information.

Question 80

What are the units of k in a first-order reaction?

A)
B) M²s
C)
D)
E)