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

Authored by Patrick Boylan

Chemistry

10th Grade

NGSS covered

Used 263+ times

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20 questions

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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

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

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

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

Tags

NGSS.HS-PS1-5

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

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

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

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

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AP CHEM Unit 5 Days 1-3 REVIEW

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!

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AP CHEM Unit 5 Days 1-3 REVIEW

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!

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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!