wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Prof temmy filtered questions on chemical kinetics

Total questions: 92

Worksheet time: 3hrs 53mins

Name
Class
Date
1.

Which of the following, when dissolved in water, would create a nonelectrolyte?

a)

C2H6O

b)

NH4NO3

c)

NaOH

d)

BaCl2

2.

You begin with a solution of 400 grams of potassium chloride dissolved in 1250 mL of water. If the volume of water is increased by 33%, what is the final molarity of the solution?

a)

3.2 M

b)

4.3 M

c)

5400 M

d)

5.4 M

3.
Which solution would be least likely to carry an electric current?
a)
NaCl
b)
HCl
c)
C6H12O6
d)
CsI
4.

HNO3

a)

strong electrolyte

b)

weak electrolyte

c)

non - electrolyte

5.

What is defined as an atom or molecule with a net electric charge due to the loss or gain of one or more electrons?

a)

Proton

b)

Conductivity

c)

Ion

d)

Electrolyte

6.

Which of the following will produce ions to conduct electricity when dissolved in water?

a)

CaCl2

b)

NH3

c)

CH4

d)

P2O5

7.
A possible rate law for a third overall order of a reaction is __________________
a)
Rate = k [A]2[B]2
b)
Rate = k [A][B]3
c)
Rate = k [A]3 [B]
d)
Rate = k [A]2[B]
8.
What is the rate exponent for A?
a)
0
b)
1
c)
2
9.
What two trials would you use to find the rate exponent for B?
a)
trials 1 and 2
b)
trials 1 and 3
c)
trails 2 and 3
10.
Which two trials would you use to find the rate exponent for A?
a)
trials 1 and 2
b)
trials 1 and 3
c)
trials 2 and 3
11.

Consider the following data for the reaction:

A+2B → C+D

Deduce the order of reaction with respect to A and with respect to B

a)

A is first order and B is second order.

b)

A is second order and B is first order.

c)

A is first order and B is first order.

d)

A is second order and B is second order.

12.

Consider the following data for the reaction:

A+2B → C+D

Work out a value for the rate constant of this reaction with units.

a)

10 mol-2dm6s-1

b)

10 mol-dm3s-1

c)

5 mol-2dm6s-1

d)

5 mol-dm3s-1

13.

Consider the following data for the reaction:

2X+4Y → Q+2R

Write the rate equation for this reaction.

 

a)

Rate = k

b)

Rate = k[X]

c)

Rate = k[X][Y]

d)

Rate = k[Y]

14.

Consider the following data for the reaction:

2X+4Y → Q+2R

What are the units of the rate constant?

   

a)

Moldm-3

b)

Mol-1dm3

c)

Mol-1s-1

d)

Mol-1dm3s-1

15.

A reaction is zero order with respect to P and second order with respect to Q. What would be the effect of doubling the concentration of P and the concentration of Q on the overall rate of reaction?

 

 

a)

Constant

b)

The rate of reaction would be Double

c)

The rate of reaction would be Triple

d)

The rate of reaction would be quadrupled

16.

The rate information below was obtained for the following reaction at a constant temperature

2NO2(g) + F2(g) -> 2NO2F(g)

What are the orders of the reaction with respect to N02 and F2?

a)

NO2 is first order and F2 is second order.

b)

N02 is second order and F2 is first order.

c)

NO2is first order and F2 is first order.

d)

NO2 is second order and F2 is zero order.

17.
For 2A + B → 2C, the rate of production of C has been found to be 12 M/s. During that reaction, the rate of reaction was?
a)
12 M/s
b)
24 M/s
c)
6 M/s
d)
Cannot tell without more data
18.
A compound has a half-life of 14 min. How much time will it take a 12 mol sample to decay to 1.5 mol?
a)
14 min
b)
28 min
c)
42 min
d)
56 min
19.

What order of reaction has a half-life that does not change regardless of the initial concentration?

a)

Zero

b)

First

c)

Second

d)

Third

20.

For second order reaction, the initial concentration of reactant A is 0.24 M. If the rate constant is 8.1 x 10-2 M-1 s-1, what is the concentration of A after 29 seconds?

a)

0.02 M

b)

0.15 M

c)

0.30 M

d)

0.45 M

21.

Given the following balanced equation :

2NO(g) + Cl2(g) → 2NOCl(g)

If the rate of disappearance of Cl2 is 4.84 x 10-2 Ms-1, what is the rate of disappearance of NO?

a)

1.45 x 10-2 Ms-1

b)

2.42 x 10-2 Ms-1

c)

3.67 x 10-2 Ms-1

d)

9.68 x 10-2 Ms-1

22.

In the chemical reaction, the successful formation of products depends on the following factors EXCEPT:

a)

The collisions between reacting molecules must be effective

b)

The colliding molecules must approach each other in the right orientation

c)

The energy of colliding molecules must be equal to or more than activation energy

d)

A collision between molecules must produce sufficient energy to overcome the activation energy

23.

The reaction A + 2B → products was found to have the rate law, k = k[A][B]2. Predict by what factor the rate of reaction will increase when the concentration of B is doubled and the concentration of A remained uncanged

a)

2

b)

4

c)

6

d)

8

24.

The first order rate constant for the decomposition of 0.5 M compound A at 100oC is 0.03 min-1. Calculate the half-life of A.

a)

1.5 min

b)

8.3 min

c)

23.1 min

d)

66.7 min

25.

The rate constant for a second order reaction at 30oC is 2.0 x 10-6 M-1s-1. The activation energy for this is 108 kJ mol-1. By using Arrhenius equation, determine the collision frequency factor, A for the reaction.

a)

5.0 x 1012

b)

6.0 x 1012

c)

8.0 x 1012

d)

1.0 x 1013

26.

Which of the following statements about catalyst is true?

a)

It does not take part in the reaction

b)

It increase the yield of the reaction

c)

It provides an alternative mechanism for the reaction

d)

It increases the number of collisions between reacting molecules per second

27.

What are the sign and units of k in the following rate law equation?

rate=k[A]2rate=k\left[A\right]^2

a)

Negative s−1s^{-1}

b)

Positive M−1s−1M^{-1}s^{-1}

c)

Negative M−1s−1M^{-1}s^{-1}

d)

Positive s−1s^{-1}

28.
The rate law for the reaction 2NO(g) + O2(g) → 2NO2(g) is first order in O2 and third order overall. What is the rate law for the reaction?
a)
Rate = k [NO]2[O2]2
b)
Rate = k [NO]1[O2]2
c)
Rate = k [NO]2[O2]1
d)
Rate = k [2NO]2[O2]1
29.

The Arrhenius law governs what relationship?

a)

temperature and rate constant k

b)

temperature and activation energy

c)

temperature and pH

d)

pH and rate constant

30.

Molecularity of Reactions: Identify the incorrect statement among the following

a)

Molecularity refers to the number of reactant particles involved in an elementary step and can only be an integer value.

b)

The molecularity of a reaction provides direct insight into the reaction mechanism, indicating how reactant molecules come together in the rate-determining step.

c)

For complex reactions, the overall reaction molecularity is the sum of the molecularities of all the elementary steps in the reaction mechanism.

31.

Temperature Dependence of Rate Constants: Identify the incorrect statement among the following

a)

According to the Arrhenius equation, a plot of ln(k) versus 1/T (where T is the temperature in Kelvin) yields a straight line with a slope of -Ea/R.

b)

The Arrhenius equation predicts that the rate constant (k) decreases as the temperature increases, showcasing the temperature's impact on reaction speed.

c)

Activation energy (Ea) and the gas constant (R) are factors in the Arrhenius equation that determine the temperature dependence of the rate constant.

32.

First-Order Reactions: Identify the incorrect statement among the following

a)

A first-order reaction's rate law is given by rate = k[A], where [A] is the concentration of the reactant, and k is the rate constant.

b)

The half-life of a first-order reaction is independent of the initial concentration of the reactants and is a constant for the reaction.

c)

In first-order kinetics, the time it takes for the reactant concentration to reduce to half its initial value is called the reaction's half-life, which varies with concentration.

33.

Order and Molecularity: Identify the incorrect statement among the following

a)

The molecularity of a reaction refers to the number of molecules participating in the rate-determining step and is always an integer.

b)

Reaction order is determined experimentally and can be any fraction, reflecting the reaction rate's dependence on reactant concentration.

c)

Both reaction order and molecularity describe the same aspect of a chemical reaction, specifically how the reaction rate changes with reactant concentration.

34.

Zero-Order Reactions: Identify the incorrect statement among the following

a)

In a zero-order reaction, the rate is dependent on the initial concentration of the reactants and varies over time.

b)

The rate law for a zero-order reaction can be expressed as rate = k, indicating that the reaction rate is directly proportional to the rate constant alone.

c)

Zero-order kinetics imply that the reaction rate changes with variations in temperature but not with changes in reactant concentrations.

35.

Determine the value of rate constant, K based on this table


Rate = K [Q]2

a)

1.0 M-1 s-1

b)

2.0 M-1 s-1

c)

3.0 M-1 s-1

d)

4.0 M-1 s-1

36.

Which of the graph, half life for zero order

a)
b)
c)
d)
37.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
38.
A possible rate law for a third overall order of a reaction is __________________
a)
Rate = k [A]2[B]2
b)
Rate = k [A][B]3
c)
Rate = k [A]3 [B]
d)
Rate = k [A]2[B]
39.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the rate law for the reaction?

a)

rate = k[NH3]

b)

rate = k[BF3]2[NH3]

c)

rate = k[BF3][NH3]

d)

rate = k[BF3][NH3]2

40.

Given the following rate law,

rate = k[A]2[B]

if [A] were doubled, what must happen to [B] to keep the rate constant?

a)

[B] must quadruple

b)

[B] must double

c)

[B] must be havled

d)

[B] must be quartered

41.

Which of the following are true of reaction rates?


I. The overall rate law is determined by the fastest step of a reaction


II. The presence of a catalyst will increase the number of molecules entering the transition state


III. An increase in temperature will increase the rate of a reaction


IV. Increasing the concentration of reactants will increase the rate at which products yield

a)

II+III+IV

b)

I+IV

c)

II + III

d)

I+II+III

42.

Units of rate is _______-

a)

M/s

b)

mol/s

c)

m.s

d)

s/M

43.

The quantity of K in rate law expression

a)

Independent of concentration

b)

Is called the Arrhenius constant

c)

Is dimensionless

d)

Is independent of temperature

44.

    Consider the reaction:2A→3B. Theaverage rate ofappearance of B is given by [B]/dt. How the average ofappearanceofB related to the average rateofdisappearanceofA?Consider\ the\ reaction:2A→3B.\ Theaverage\ rate\ ofappearance\ of\ B\ is\ given\ by\ [B]/dt.\ How\ the\ average\ ofappearanceofB\ related\ to\ the\ average\ rateofdisappearanceofA?  

a)

                              −2[A])/3t-2[A])/3t  

b)

[A]/t[A]/t        

c)

−[A])/t-[A])/t  

d)

−3[A])/2t-3[A])/2t  

45.

Based on the collision model, the atoms in the top of potential energy ‘’hill’’ are called

a)

Top of hill

b)

Activation energy

c)

Transition state

d)

Steric factor

46.

For a certain reaction, the rate=k[NO]2[O2],when the initial concentration of NO is tripled,the initial rate−For\ a\ certain\ reaction,\ the\ rate=k[NO]2[O2],when\ the\ initial\ concentration\ of\ NO\ is\ tripled,the\ initial\ rate-  

a)

 Decreases by a factor of nine

b)

Increase by a factor of six

c)

 Increase by a factor of nine

d)

Decreases by a factor of six

47.

The half-life period of a first-order process

a)

Depends on reactant concentration raised to the first power

b)

Is inversely proportional to square of reactant concentration

c)

Is inversely proportional to reactant concentration

d)

Is totally independent of reactant concentration

48.

rate = k[A]

The rate constant in the rate law above is 0.5 L/mol·s. If the initial concentration of A is 0.1 M, how long will it take for [A] to drop to 0.025 M?

a)

0.7 s

b)

1.4 s

c)

2.8 s

d)

There is not enough information given.

49.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
50.
What would be my the overall order of this rate law? 
Rate=[A]2[B]1
a)
0 Order
b)
1st Order
c)
2nd Order
d)
3rd Order
51.
If my rate law is second order and I increase my concentration to 4, what would my new rate be? 
a)
4
b)
16
c)
2
d)
8
52.

Arrhenius equation is

a)

k = AeEa/RT

b)

k = Ae-Ea/RT

c)

k = AeRT/Ea

d)

k = Ae-RT/Ea

53.

The unit of rate and rate constant are same for ______order reaction

a)

zero

b)

one

c)

two

d)

three

54.

The rate law of the reaction 2N2O5 → 2NO2 + O2 is

a)

r = k[N2O5 ]

b)

r = k[N2O5 ]2

c)

r = k[N2O5 ]0

d)

r = k[NO2]4 [O2]

55.

Consider this reaction:

2SO2(g) + O2(g) →\rightarrow   2SO3(g)

The rate of disappearance of SO2 is 1.6 gL-1 min-1. What is the rate of formation of SO3 in molL-1min-1? [Molar mass SO2: 64.0 gmol-1]

a)

0.035

b)

0.025

c)

0.120

d)

0.050

56.

For the reaction, A(g) + B(g) →\rightarrow   2C(g), the rate equation is:

Rate = k[A]2[B]

If the concentration of reactant A is increase by triple at constant temperature, by what factor will the rate of reaction change?

a)

2 

b)

6

c)

4

d)

9

57.

The rate constant is doubles on the increasing temperature from 310K to 350K. What is the activation energy (in kJ mol-1) for this reaction?

a)

12.3

b)

15.6

c)

25.8

d)

29.2

58.

An endothermic reaction with high activation energy for the forward reaction is given by the diagram.

a)

A

b)

B

c)

C

d)

D

59.
Which of the following is expressions represents correctly rate of following reaction?
X + Y → Z + Q     ΔH = +22kj/mol
a)
Rate = +Δ[X] / Δt
b)
Rate = +Δ[Y] / Δt
c)
Rate = +Δ[Z] / Δt
d)
Rate = -Δ[Q] / Δt
60.

Which sample of HCl(aq) reacts at the fastest rate with a 1.0-gram sample of iron filings?

a)

10 mL of 1 M HCl(aq) at 10°C

b)

10 mL of 1 M HCl(aq) at 25°C

c)

10 mL of 3 M HCl(aq) at 10°C

d)

10 mL of 3 M HCl(aq) at 25°C

61.

A 5.0-gram sample of zinc and a 50.-milliliter sample of hydrochloric acid are used in a chemical reaction. Which combination of these samples has the fastest reaction rate?

a)

a zinc strip and 1.0 M HCl(aq)

b)

a zinc strip and 3.0 M HCl(aq)

c)

zinc powder and 1.0 M HCl(aq)

d)

zinc powder and 3.0 M HCl(aq)

62.

The rate constant of a reaction is 5.8 ×\times 10 M-1s-1. The order of the reaction is...

a)

0th order

b)

1st order

c)

2nd order

d)

3rd order

63.

What is the half-life (t1/2) of a reactant with a decay constant (λ)\left(\lambda\right) of 0.693?

a)

1

b)

2

c)

3

d)

4

64.

rate = k[A]

The rate constant in the rate law above is 0.5 1/s. If the initial concentration of A is 0.1 M, how long will it take for [A] to drop to 0.025 M?

a)

0.7 s

b)

1.4 s

c)

2.8 s

d)

There is not enough information given.

65.
Which two trials would you use to find the rate exponent for A?
a)
trials 1 and 2
b)
trials 1 and 3
c)
trials 2 and 3
66.
What is the rate exponent for A?
a)
0
b)
1
c)
2
67.
The reaction
2ClO2(aq) + 2OH-(aq) —> ClO3(aq) + ClO2-(aq) + H2O(l) was studied with the following results: 
Calculate the rate constant with proper units. 
a)
230 M/S
b)
230 M-S-
c)
230 M2-S-
d)
R=K[ClO2][OH-]
68.
Find the order for F2 and CIO2 using data shown below.
a)
(F2 - 2nd order) (CIO2 - 1st order)
b)
(F2 - 1st order) (CIO2 - 1st order)
c)
(F2 - 1st order) (CIO2 - 2nd order)
d)
(F2 - 2nd order) (CIO2 - 2nd order)
69.
A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to __________. 
a)
increase by a factor of 27 
b)
increase by a factor of 9 
c)
triple 
d)
decrease by a factor of the cube root of 3  
70.

A → products

The reactant A in the equation above was found to be first order. Which of the following integrated rate laws would correspond to this reaction?

a)

1/[A] = kt + 1/[A]o

b)

ln[A] = -kt + ln[A]o

c)

[A] = -kt + [A]o

71.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
72.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
73.

For the following reaction

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

74.

For the following reaction

2 N2O5(g) → 4 NO2(g) + O2(g) what is the relationship between the rate of consumption of N2O5 and that of appearance of O2?

a)

1/2 Δ[N2O5]/Δt = Δ[O2]

b)

-1/2 Δ[N2O5]/Δt = Δ[O2]

c)

-Δ[N2O5]/Δt = 1/2 Δ[O2]

d)

-Δ[N2O5]/Dt = Δ[O2]

75.
An unknown salt, M2Z, has a Ksp of 3.3 x 10-9. Calculate the solubility in mol/L of M2Z.
a)
2.9 x 10-5 M
b)
5.7 x 10-5 M
c)
9.4 x 10-5 M
d)
3.7 x 10-5 M
76.
The molar solubility of PbI2 is 1.52 x 10-3 M. Calculate the value of Ksp for PbI2.
a)
3.51 x 10-9
b)
1.40 x 10-8
c)
4.62 x 10-6
d)
1.52 x 10-3
77.
Calculate the [H+] in a solution that has a pH of 2.73.
a)
5.4 x 10-12 M
b)
1.9 x 10-3 M
c)
2.7 M
d)
11.3 M
78.
The pH at the equivalence point of the titration of a strong acid with a strong base is:
a)
3.9
b)
4.5
c)
7.0
d)
8.2
79.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
80.
Silver chromate, Ag2CrO4, has a Ksp of 8.96 x 10-12. Calculate the solubility in mol/L of silver chromate.
a)
1.31 x 10-4M
b)
1.65 x 10-4M
c)
2.25 x 10-12M
d)
2.08 x 10-4M
81.
The pH of a solution at 25ₒC in which [OH-] = 3.9 x 10-5M is:
a)
4.41
b)
3.90
c)
9.59
d)
4.80
82.
The solubility of CaSO4 in pure water at 0ₒC is 1.14 g/L. The value of the solubility product is
a)
8.37 x 10-3
b)
1.14 x 10-3
c)
9.15 x 10-2
d)
7.01 x 10-5
83.
A weak acid, HF, is in solution with dissolved sodium fluoride, NaF. If HCl is added, which ion will react with the extra hydrogen ions from the HCl to keep the pH from changing?
a)
OH-
b)
Na+
c)
F-
d)
Na-
84.
The correct mathematical expression for finding the molar solubility (s) of Sn(OH)2 is:
a)
2s2 = Ksp
b)
2s3 = Ksp
c)
4s3 = Ksp
d)
8s3 = Ksp
85.
An unknown salt, M2Z, has a Ksp of 3.3 x 10-9. Calculate the solubility in mol/L of M2Z.
a)
2.9 x 10-5 M
b)
5.7 x 10-5 M
c)
9.4 x 10-5 M
d)
3.7 x 10-5 M
86.

Write the solubility product constant expression for:

AgCl

(a)  

87.

Which salt is least soluble?

a)
AgCl
b)
BaSO₄
c)
PbI₂
d)
ZnCO₃
88.

Which salt is most soluble?

a)
AgCl
b)
BaSO₄
c)
PbI₂
d)
ZnCO₃
89.

What is the solubility in moles/liter of AgBr if the Ksp = 5.0 x 10⁻¹³?

(a)  

90.

If the solubility of Li₂CO₃ = 0.15 moles/liter, what is its Ksp at this temperature?

(a)  

91.

The solubility product of silver chromate (VI) at room temperature is 2.4 x 10-12. Calculate the molar solubility of Ag+(aq) and CrO42-(aq) ions in a saturated solution of silver chromate (VI) at room temperature.

a)

Ag+ = 1.68 x 104 M and CrO42- = 8.4 x 10-5 M

b)

Ag+ = 1.68 x 104 M and CrO42- = 8.4 x 105 M

c)

Ag+ = 1.68 x 10-4 M and CrO42- = 8.4 x 105 M

d)

Ag+ = 1.68 x 10-4 M and CrO42- = 8.4 x 10-5 M

92.

The Ksp value for PbF2 is 4 x 10-8. Calculate the molar solubility of solid PbF2 in a 0.5M NaF solution.

a)

8 x 108

b)

1.6 x 107

c)

8 x 10-8

d)

1.6 x 10-7

Similar Resources on Wayground

EXAMEN CONOCIMIENTOS SEMANA 5

93 questions

EXAMEN CONOCIMIENTOS SEMANA 5

quiz

Worksheet

•

University

AP Chemistry Thou Shalt Not Forget

90 questions

AP Chemistry Thou Shalt Not Forget

quiz

Worksheet

•

11th Grade - University

Unit 1 Review

88 questions

Unit 1 Review

quiz

Worksheet

•

10th Grade - University

Spring Final Exam Chemistry 2025

90 questions

Spring Final Exam Chemistry 2025

quiz

Worksheet

•

10th Grade - University

CHEM 1114 Final Exam Practice Quiz Spring 2022

95 questions

CHEM 1114 Final Exam Practice Quiz Spring 2022

quiz

Worksheet

•

University

pt2 -chem

89 questions

pt2 -chem

quiz

Worksheet

•

University

EXAM 3-1

90 questions

EXAM 3-1

quiz

Worksheet

•

University

Conceptos fundamentales de Termodinámica

93 questions

Conceptos fundamentales de Termodinámica

quiz

Worksheet

•

University