In any first order reaction, as the reaction proceeds at constant temperature, which describes the corresponding effects on k (the rate constant) and rate?

k remains the same; rate decreases

k and rate both remain the same

k remains the same; rate increases

k decreases; rate remains the same

lowers the amount of energy added to a reaction

should be eliminated when we solve elementary reaction steps of a proposed reaction mechanism simultaneously

should always be introduced and eliminated in the first elementary step of a proposed reaction mechanism

lowers the amount of energy released by an exothermic reaction

Increasing temperature of a chemical reaction:

increases the number of collisions per second of chemical reactants

increases the speed of reaction

can increase the pressure of reactants

Multi-step (Consecutive) Reactions: Mechanisms in which one elementary step is followed by another are very common. step 1: A + B → Q step 2: B + Q → C net reaction: A + 2B → C Which of the following is false?

Intermediates such as Q can appear in the rate law of a net reaction.

The net reaction is just the sum of its elementary steps.

The species Q is an intermediate, usually an unstable or highly reactive species.

If both steps proceed at similar rates, rate law experiments on the net reaction would not reveal that two separate steps are involved here.The rate law for the reaction would be rate=k[A][B ]2

The rate law for a reaction is rate = k [A][B]2 Which one of the following statements is false?

D) The reaction is second order overall.

A) If [B] is doubled, the reaction rate will increase by a factor of 4.

B) The reaction is second order in B.

C) The reaction is first order in A.

C 12 H 22 O 11 (aq)+H2O(l)→2C 6 H 12 O 6 (aq) The chemical equation shown above represents the hydrolysis of sucrose. Under certain conditions, the rate is directly proportional to the concentration of sucrose. Which statement supports how a change in conditions can increase the rate of this reaction?

Increasing the concentration of sucrose will increase the rate of hydrolysis by increasing the frequency of the collisions between the sucrose and the water molecules.

Increasing the amount of water in which the sugar is dissolved will increase the frequency of collisions between the sucrose molecules and the water molecules resulting in an increase in the rate of hydrolysis.

Decreasing the temperature will increase the frequency of the collisions between the sucrose molecules and the water molecules resulting in an increase in the rate of hydrolysis.

Decreasing the concentration of sucrose will increase the rate of hydrolysis by increasing the frequency of the collisions between the sucrose and the water molecules.

Zn(s)+2 HCl(aq)→ZnCl2(aq)+H2(g) Zn(s) reacts with HCl(aq) according to the equation shown above. In trial 1 of a kinetics experiment, a 5.0g piece of Zn(s) is added to 100mL of 0.10MHCl(aq). The rate of reaction between Zn(s) and HCl(aq) is determined by measuring the volume of H2(g) produced over time. In trial 2 of the experiment, 5.0g of powdered Zn(s) is added to 100mL of 0.10MHCl(aq). Which trial will have a faster initial rate of reaction and why?

Trial 2, because the sample of Zn(s) Zn(s) has a greater surface area for the reaction to take place.

Trial 1, because there is a higher concentration of Zn(s) Zn(s) in the reaction mixture.

Trial 1, because the sample of Zn(s) Zn(s) has less surface area for the reaction to take place.

Trial 2, because there is a higher concentration of HCl(aq) HCl(aq) in the reaction mixture.

CH 3 I+NaOH→CH 3 OH+NaI The rate of the reaction represented by the chemical equation shown above is expressed as rate=k[CH 3 I][NaOH]. Based on this information, which of the following claims is correct?

The rate of the reaction will double if the concentration of CH3I is doubled while keeping the concentration of NaOH constant

The reaction will proceed at a slower rate with increasing temperature.

The rate of the reaction will double when the concentrations of both CH3I and NaOH are doubled.

A larger amount of CH3OH will be produced if the concentrations of CH3I and NaOH are halved.

Step 1: H2O2+I−→IO−+H2O Step 2: H2O2+IO−→H2O+O2+I− The mechanism for a chemical reaction is shown above. Which of the following statements about the overall reaction and rate laws of the elementary reactions is correct?

The chemical equation for the overall reaction is 2 H2O2→2 H2O+O2 , and the rate law for elementary step 1 is rate=k[H2O2][I−] .

The chemical equation for the overall reaction is 2 H2O2+I−→ 2 H2O+O2+I− , and the rate law for elementary step 2 is rate=k[H2O2][IO−] .

The chemical equation for the overall reaction is H2O2+IO−→ H2O+O2+I− , and the rate law for elementary step 2 is rate=k[H2O2]2[IO−] .

The chemical equation for the overall reaction is 2 H2O2→2 H2O+O2 , and the rate law for elementary step 1 is rate=k[H2O2]2 .

Step 1: N2O5→NO2+NO3 (slow) Step 2: NO2+NO3→NO2+NO+O2 (fast) Step 3: NO+N2O5→3 NO2 (fast) A proposed reaction mechanism for the decomposition of N2O5(g) is shown above. Based on the proposed mechanism, which of the following correctly identifies both the chemical equation and the rate law for the overall reaction?

The chemical equation for the overall reaction is 2N2O5(g)→4NO2(g)+O2(g) , and the rate law is rate=k[N2O5] .

The chemical equation for the overall reaction is NO(g)+N2O5(g)→3NO2(g) , and the rate law is rate=k[NO][N2O5] .

The chemical equation for the overall reaction is 2N2O5(g)→4NO2(g)+O2(g) , and the rate law is rate=k[N2O5]2 .

The chemical equation for the overall reaction is N2O5(g)+NO(g)+NO3(g)→4NO2(g)+O2(g) , and the rate law is rate=k[N2O5][NO][NO3] .

The two diagrams above represent collisions that take place at the same temperature between a CO molecule and an NO2 molecule. The products are CO2 and NO. Which diagram most likely represents an effective collision, and why?

Diagram 1 represents an effective collision because the two molecules have the proper orientation to form a new C−O bond as long as they possess enough energy to overcome the activation energy barrier.

Diagram 1 represents an effective collision because the molecules have about the same size and the same energy, which leads to a larger rate constant (k).

Diagram 2 represents an effective collision because the molecules are aligned head-to-head and that maximizes the overlap between their atomic orbitals, forming more products.

Diagram 2 represents an effective collision because the oxygen atoms are the most electronegative and will minimize their repulsions when oriented away from each other.

The diagram above shows the distribution of molecular energies for equimolar samples of a reactant at different temperatures. Based on the diagram, at which temperature will the reactant be consumed at the fastest rate, and why?

At T4 , because a larger fraction of the molecules have an energy that is equal to or greater than the activation energy.

At T3 , because at this temperature the rate of consumption for about half of the molecules is determined by their orientation.

At T2 , because at this temperature most of the molecules undergo collisions frequently.

At T1 , because a larger fraction of the molecules have about the same energy.

AP Chemistry Collision

Quiz

•

Chemistry

•

11th Grade

•

Practice Problem

•

Hard

•

NGSS

HS-PS1-5, HS-PS1-4, HS-PS1-2

+2

Standards-aligned

Charles Martinez

FREE Resource

25 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Which one of the following is a first order, overall reaction

k₁= 1.000 M s^-1

k₁= 5403.2 M^½ s^½

k₁= 1.23 x 10^-6 M^-1 s^-1

k₁= 10.7 s^-1

Tags

NGSS.HS-PS1-5

2.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

A. is most exothermic

B. is most exothermic

C. is most exothermic

D. is most exothermic

Tags

NGSS.HS-PS1-4

3.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

Consider the following rate law: Rate = k[A]ⁿ[B]^m
How are the exponents n and m determined?

by using balanced chemical equation

By using the subscripts for the formulas

By educated guess

By experiment

4.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

A. has largest E_a

B. has largest E_a

C. has largest E_a

E. has largest E_a

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

5.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

A. is the slowest reaction

B. is the slowest reaction

C. is the slowest reaction

E. is the slowest reaction

Tags

NGSS.HS-PS1-4

NGSS.HS-PS1-5

6.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

step 1: O₃ → O₂ + O
step 2: O₃ + O → 2 O₂
The oxygen atom (O) is considered to be a(n)...

reactant

catalyst

reaction intermediate

activated complex

7.

MULTIPLE CHOICE QUESTION

15 mins • 1 pt

The reaction of (CH₃)₃CBr with hydroxide ion proceeds:
(CH₃)₃CBr(aq) + OH^-(aq) → (CH₃)₃COH(aq) + Br^-(aq)
What will the initial rate (in mol/L*s) be in Experiment 4?

0.003

0.006

0.009

0.018

Tags

NGSS.HS-PS1-5

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AP Chemistry Collision

25 questions

Which one of the following is a first order, overall reaction

Consider the following rate law: Rate = k[A]n[B]mHow are the exponents n and m determined?

step 1: O3 → O2 + Ostep 2: O3 + O → 2 O2The oxygen atom (O) is considered to be a(n)...

The reaction of (CH3)3CBr with hydroxide ion proceeds:(CH3)3CBr(aq) + OH-(aq) → (CH3)3COH(aq) + Br-(aq)What will the initial rate (in mol/L*s) be in Experiment 4?

In any first order reaction, as the reaction proceeds at constant temperature, which describes the corresponding effects on k (the rate constant) and rate?

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?

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Discover more resources for Chemistry

Consider the following rate law: Rate = k[A]ⁿ[B]^m
How are the exponents n and m determined?

step 1: O₃ → O₂ + O
step 2: O₃ + O → 2 O₂
The oxygen atom (O) is considered to be a(n)...

The reaction of (CH₃)₃CBr with hydroxide ion proceeds:
(CH₃)₃CBr(aq) + OH^-(aq) → (CH₃)₃COH(aq) + Br^-(aq)
What will the initial rate (in mol/L*s) be in Experiment 4?