A student collects the following kinetics data for a reaction. Based on the data, how would you classify the reaction? Why? NO calculator!

First Order. Concentration is halved after 3.00 min and again after another 3.00min. Thus the half-life of the reaction is constant, so the reaction is first order.

Zero Order. Concentration is halved after 3.00 min and again after another 3.00min. Thus the half-life of the reaction is constant, so the reaction is zero order.

Second Order. Concentration is halved after 3.00 min and again after another 3.00min. Thus the half-life of the reaction is constant, so the reaction is second order.

First Order. ln(Concentration) is halved after 3.00 min and again after another 3.00min. Thus the half-life of the reaction is constant, so the reaction is first order.

Why does a mixture of hydrogen and oxygen in a balloon not spontaneously explode at room temperature?

None of the molecules have a kinetic energy that is higher than or equal to the activation energy of the reaction.

It will eventually explode, you just have to wait.

The mixture is not explosive, even at high temperatures.

The reaction is already at equilibrium.

Collision theory states that

molecules must collide with the proper orientation in order to react.

all reactions become faster at lower temperature.

transition states are high energy.

The principal reason for the increase in reaction rate with increasing temperature is

the fraction of high energy molecules increases with increasing temperature.

the pressure exerted by reactant molecules increases.

the activation energy increases with increasing temperatures.

molecules collide less frequently at high temperatures.

In order for a successful reaction to occur in the illustration provided, which of the following must occur?

The N atom in the NO molecule must strike a specific O atom in the O 3 molecule.

The N atom in the NO molecule must strike any O atom in the O 3 molecule.

The O atom in the NO molecule must strike a specific O atom in the O 3 molecule.

The O atom in the NO molecule must strike any O atom in the O 3 molecule.

AP CHEM Unit 5 Days 1-3 REVIEW

Quiz

•

Chemistry

•

10th Grade

•

Practice Problem

•

Easy

•

NGSS

HS-PS1-5, HS-PS1-7, HS-PS1-2

Standards-aligned

Patrick Boylan

Used 263+ times

FREE Resource

20 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

In general, which does NOT increase the speed of a combustion reaction?

high activation energy

adding a catalyst

increasing the amount of fuel present

increasing the temperature of the reaction

increasing surface area

Tags

NGSS.HS-PS1-5

2.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

The rate of formation of NO₂(g) in the reaction
2 N₂O₅(g) → 4 NO₂(g) + O₂(g)
is 5.78 (mol NO₂)/L/s. What is the rate at which N₂O₅ decomposes?
NO CALCULATOR

5.78
(mol N₂O₅)/L/s

2.89
(mol N₂O₅)/L/s

0.723
(mol N₂O₅)/L/s

11.6
(mol N₂O₅)/L/s

Tags

NGSS.HS-PS1-7

3.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

Which of the following is one way to correctly describe the rate of the reaction shown?

A

B

C

D

Tags

NGSS.HS-PS1-5

4.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

For the reaction
2A + B → products
use the experimental data provided to determine the rate law.
NO CALCULATOR

rate = k [A] [B]

rate = k [A] [B]⁰

rate = k [A]

rate = k [A]²

Tags

NGSS.HS-PS1-5

5.

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

Calculate the value of the specific rate constant WITH CORRECT UNITS using the data provided.
YES CALCULATOR

0.491M^-1min^-1

0.327M^-1min^-1

0.327M^-2min^-1

0.491M^-2min^-1

Tags

NGSS.HS-PS1-5

6.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

Which of the following values correspond to the values of the reaction orders x and y for NO and H₂?

x=2, y=1

x=1, y=1

x=2, y=2

x=1, y=2

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-7

7.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

What is the overall order of reaction based on the experimental data provided?

first order

second order

third order

zero order

Tags

NGSS.HS-PS1-5

Create a free account and access millions of resources

Create resources

Host any resource

Get auto-graded reports

Continue with Google

Continue with Email

Continue with Classlink

Continue with Clever

or continue with

Microsoft

Apple

Others

Already have an account?

Similar Resources on Wayground

0 questions

Chem Exam Review (Spring)

Quiz

•

0 questions

Unit 5 Vocabulary

Quiz

•

0 questions

AP Chemistry Overview

Quiz

•

0 questions

Chemical Reactions - Unit Review

Quiz

•

0 questions

AP Unit 4: Chemical Reactions

Quiz

•

Popular Resources on Wayground

5 questions

This is not a...winter edition (Drawing game)

Quiz

•

1st - 5th Grade

15 questions

4:3 Model Multiplication of Decimals by Whole Numbers

Quiz

•

5th Grade

25 questions

Multiplication Facts

Quiz

•

5th Grade

10 questions

The Best Christmas Pageant Ever Chapters 1 & 2

Quiz

•

4th Grade

12 questions

Unit 4 Review Day

Quiz

•

3rd Grade

10 questions

Identify Iconic Christmas Movie Scenes

Interactive video

•

6th - 10th Grade

20 questions

Christmas Trivia

Quiz

•

6th - 8th Grade

18 questions

Kids Christmas Trivia

Quiz

•

KG - 5th Grade

Discover more resources for Chemistry

20 questions

Periodic Trends

Quiz

•

10th Grade

29 questions

Physical or Chemical Changes

Quiz

•

9th - 10th Grade

20 questions

Periodic Table & Trends

Quiz

•

10th Grade

20 questions

Electron Configuration

Quiz

•

10th - 12th Grade

20 questions

Naming Compounds: Basic Ionic and Covalent Naming

Quiz

•

9th - 12th Grade

20 questions

Balancing Chemical Equations

Quiz

•

10th - 12th Grade

65 questions

Midterm Review Chem

Quiz

•

9th - 12th Grade

12 questions

Half-Life Calculations-More Practice

Quiz

•

9th - 12th Grade

AP CHEM Unit 5 Days 1-3 REVIEW

20 questions

In general, which does NOT increase the speed of a combustion reaction?

The rate of formation of NO₂(g) in the reaction
2 N₂O₅(g) → 4 NO₂(g) + O₂(g)
is 5.78 (mol NO₂)/L/s. What is the rate at which N₂O₅ decomposes?
NO CALCULATOR

Which of the following is one way to correctly describe the rate of the reaction shown?

For the reaction
2A + B → products
use the experimental data provided to determine the rate law.
NO CALCULATOR

Calculate the value of the specific rate constant WITH CORRECT UNITS using the data provided.
YES CALCULATOR

Which of the following values correspond to the values of the reaction orders x and y for NO and H₂?

What is the overall order of reaction based on the experimental data provided?

Consider the equation for the decomposition of N₂O₅(g) and the experimentally determined rate law below.
2N₂O₅(g)⇌ 4NO₂(g) + O₂(g)
rate=k[N₂O₅]
What are the units for the rate constant, k, with the time measured in minutes?

For the reaction shown below a series of trials were performed and the corresponding rate information was collected.
BrO₃^- + 5Br^- + 6H⁺ → 3 Br₂ + 3H₂O
What is the overall order of reaction?
NO CALCULATOR!

For the reaction shown below a series of trials were performed and the corresponding rate information was collected.
BrO₃^- + 5Br^- + 6H⁺ → 3 Br₂ + 3H₂O
For experiment 4, calculate the concentration of BrO₃^- remaining after 75% of the H⁺ has been consumed.
YES CALCULATOR!

Create a free account and access millions of resources

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

AP CHEM Unit 5 Days 1-3 REVIEW

20 questions

In general, which does NOT increase the speed of a combustion reaction?

The rate of formation of NO2(g) in the reaction2 N2O5(g) → 4 NO2(g) + O2(g) is 5.78 (mol NO2)/L/s. What is the rate at which N2O5 decomposes? NO CALCULATOR

Which of the following is one way to correctly describe the rate of the reaction shown?

For the reaction 2A + B → products use the experimental data provided to determine the rate law.NO CALCULATOR

Calculate the value of the specific rate constant WITH CORRECT UNITS using the data provided.YES CALCULATOR

Which of the following values correspond to the values of the reaction orders x and y for NO and H2?

What is the overall order of reaction based on the experimental data provided?

Consider the equation for the decomposition of N2O5(g) and the experimentally determined rate law below.2N2O5(g) ⇌ 4NO2(g) + O2(g)rate=k[N2O5]What are the units for the rate constant, k, with the time measured in minutes?

For the reaction shown below a series of trials were performed and the corresponding rate information was collected.BrO3- + 5Br- + 6H+ → 3 Br2 + 3H2OWhat is the overall order of reaction?NO CALCULATOR!

For the reaction shown below a series of trials were performed and the corresponding rate information was collected.BrO3- + 5Br- + 6H+ → 3 Br2 + 3H2OFor experiment 4, calculate the concentration of BrO3- remaining after 75% of the H+ has been consumed.YES CALCULATOR!

Create a free account and access millions of resources

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

The rate of formation of NO₂(g) in the reaction
2 N₂O₅(g) → 4 NO₂(g) + O₂(g)
is 5.78 (mol NO₂)/L/s. What is the rate at which N₂O₅ decomposes?
NO CALCULATOR

For the reaction
2A + B → products
use the experimental data provided to determine the rate law.
NO CALCULATOR

Calculate the value of the specific rate constant WITH CORRECT UNITS using the data provided.
YES CALCULATOR

Which of the following values correspond to the values of the reaction orders x and y for NO and H₂?

Consider the equation for the decomposition of N₂O₅(g) and the experimentally determined rate law below.
2N₂O₅(g)⇌ 4NO₂(g) + O₂(g)
rate=k[N₂O₅]
What are the units for the rate constant, k, with the time measured in minutes?

For the reaction shown below a series of trials were performed and the corresponding rate information was collected.
BrO₃^- + 5Br^- + 6H⁺ → 3 Br₂ + 3H₂O
What is the overall order of reaction?
NO CALCULATOR!

For the reaction shown below a series of trials were performed and the corresponding rate information was collected.
BrO₃^- + 5Br^- + 6H⁺ → 3 Br₂ + 3H₂O
For experiment 4, calculate the concentration of BrO₃^- remaining after 75% of the H⁺ has been consumed.
YES CALCULATOR!