Which of the following best describes why increasing temperature increase reaction rate?

Collisions become more frequent and more energetic.

Collisions become more frequent.

Collisions become more energetic.

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?

There is not enough information given.

What two factors govern whether a collision between reacting particles will be effective?

orientation and potential energy

potential energy and kinetic energy

Under the collision theory, the particles must collide with ____ and ____ for a reaction to occur.

sufficent energy and correct orientation

sufficient rate and sufficient energy

sufficient surface area and correct orientation

sufficient catalyst and sufficient energy

Decreasing the particle size increases the reaction rate because

It increases the number of collisions

It increases the likelihood of collisions with the correct geometry

It decreases the surface area available to react

Grinding a seltzer tablet into powder increases the rate of reaction due to...

increased concentration of reactants

better orientation of reactants

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

To slow down a chemical reaction you will do one of the following:

Place the reactants in a ice bath

Place the reactants in hot water

Keep stirring the reactants with a stirring rod

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

How does pressure affect reaction rate?

Increased pressure increases reaction rate because particles collide more frequently

Increased pressure increases reaction rate because particles collide less frequently

Decreased pressure increases reaction rate because particles collide more frequently

Decreased pressure increases reaction rate because particles collide less frequently.

How does concentration affect reaction rate

In a first order or higher reaction, higher concentration increases the reaction rate because particles collide more frequently

In all reactions, higher concentration increases the reaction rate because particles collide more frequently

In all reactions, lower concentration increases the reaction rate because particles collide more frequently

In a first order or higher reaction, lower concentration increases the reaction rate because particles collide more frequently.

Overall reaction order can be determined how?

Adding the powers to which reactant concentrations are raised in the rate law

Multiplying the powers to which reactant concentrations are raised in the rate law

Subtracting the powers to which reactant concentrations are raised in the rate law

Dividing the powers to which reactant concentrations are raised in the rate law.

Excess magnesium powder was added to a beaker containing hydrochloric acid, HCl (aq). The mass of the beaker and its contents was recorded and plotted against time (line I). Which change could give line II?

Using the same volume of more concentrated HCl

Doubling the mass of powdered Mg

Using the same mass of Mg ribbon

The diagram represents the Maxwell‒Boltzmann energy distribution curve of the reactants for a chemical reaction with different activation energies, E a1 and E a2 . What is the reason why the rate of the reaction with activation energy E a2 is greater?

More frequent collisions between the particles occur.

More energetic collisions between the particles occur.

Which group of particles shows that increasing surface area increases collisions among particles?

Cannot be determined by either picture

At higher temperature, 2000K, the curve is shifted to the right. Which of the following is true ?

fraction of molecules with energy > E a increases

fraction of molecules with energy > E a decreases

Which of the following is FALSE for Maxwell Boltzmann distribution curve?

At higher temp, area under curve is greater than at low temp

Area under curve represent number of particles

Increase in temperature will shift the curve to right

High temp, fraction of molecules with energy > E a increases

On a Maxwell-Boltzmann distribution curve, a suitable label for the y-axis is

Fraction of particles with Kinetic Energy (E)

Chemical Kinetics

Authored by Charles Martinez

Chemistry

11th - 12th Grade

NGSS covered

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60 questions

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MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which of the following plots will show a linear relationship for a second order reaction?

[A] vs time

¹/_[A] vs time

ln[A] vs time

[A]² vs time

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

The iodide ion reacts with hypochlorite ion in the following way:
OCl^- + I^-⟶ OI^- + Cl^-.
This rapid reaction gives the rate data shown. What is the rate law?

rate = [OCl^-]²[I^-]

rate = [OCl^-][I^-]²

rate = [OCl^-][I^-]

rate = [OCl^-]

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

1 min • 1 pt

The following data were measured for the reaction
BF₃(g) + NH_3(g) ⟶ F₃BNH_3(g)
What is the rate law for the reaction?

rate = k[NH₃]

rate = k[BF₃]²[NH₃]

rate = k[BF₃][NH₃]

rate = k[BF₃][NH₃]²

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

The following data were measured for the reaction
BF_3(g) + NH_3(g) ⟶ F₃BNH_3(g)
What is the rate when [BF₃] = 0.100 M and [NH₃] = 0.500 M ?

.01704 M/s

.0852 M/s

.1704 M/s

.852 M/s

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

1 min • 1 pt

A reaction is found to be second order with respect to carbon monoxide. If the concentration of carbon monoxide is doubled, the rate of reaction __________.

doubles

remains unchanged

increases by a factor of 4

is reduced by a factor of 2

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What letter represents the activation energy?

Tags

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Given the following rate law,
rate = k[A]²[B]
if [A] were doubled, what must happen to [B] to keep the rate constant?

[B] must quadruple

[B] must double

[B] must be havled

[B] must be quartered

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Chemical Kinetics

Which of the following plots will show a linear relationship for a second order reaction?

The iodide ion reacts with hypochlorite ion in the following way:OCl- + I- ⟶ OI- + Cl-.This rapid reaction gives the rate data shown. What is the rate law?

The following data were measured for the reaction BF3(g) + NH3(g) ⟶ F3BNH3(g)What is the rate law for the reaction?

The following data were measured for the reactionBF3(g) + NH3(g) ⟶ F3BNH3(g)What is the rate when [BF3] = 0.100 M and [NH3] = 0.500 M ?

A reaction is found to be second order with respect to carbon monoxide. If the concentration of carbon monoxide is doubled, the rate of reaction __________.

What letter represents the activation energy?

Given the following rate law, rate = k[A]2[B]if [A] were doubled, what must happen to [B] to keep the rate constant?

Which of the following best describes why increasing temperature increase reaction rate?

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?

Which species is the catalyst in this reaction mechanism?

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The iodide ion reacts with hypochlorite ion in the following way:
OCl^- + I^-⟶ OI^- + Cl^-.
This rapid reaction gives the rate data shown. What is the rate law?

The following data were measured for the reaction
BF₃(g) + NH_3(g) ⟶ F₃BNH_3(g)
What is the rate law for the reaction?

The following data were measured for the reaction
BF_3(g) + NH_3(g) ⟶ F₃BNH_3(g)
What is the rate when [BF₃] = 0.100 M and [NH₃] = 0.500 M ?

Given the following rate law,
rate = k[A]²[B]
if [A] were doubled, what must happen to [B] to keep the rate constant?

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?