How does increasing the surface area affect the rate of a chemical reaction?

Increases the rate by increasing collisions

Decreases the rate by reducing collisions

Has no effect on the rate of reaction

Decreases the rate by increasing the distance between reactant molecules

What effect does agitation have on the rate of a chemical reaction?

Increases the rate by dispersing the reactants more evenly

Decreases the rate by decreasing the energy of the system

Decreases the rate by reducing reactant concentration

Has no effect on the rate of reaction

According to the Collision Theory, what is the first condition that must be met for a reaction to occur?

The reactants come into contact.

The reactants must be in a liquid state.

The reactants must be heated to a certain temperature.

The reactants must be of opposite charges.

What is required for the reactants to successfully react according to the Collision Theory?

They must collide with a certain minimum energy.

They must be in a gaseous state.

They must be catalyzed by an enzyme.

What does the Collision Theory state about the molecular orientation during a reaction?

It must be in 3-dimensional space with the correct molecular orientation.

It must be in 2-dimensional space.

It does not matter as long as energy is sufficient.

What generally happens to the rate of a chemical reaction as time progresses?

It generally slows down because the concentration of the reactants decreases.

It increases as the concentration of reactants increases.

It remains constant throughout the reaction.

It speeds up due to the formation of more products.

What could cause a chemical reaction to stop?

All reactants are used up or the system has reached equilibrium.

The temperature of the system decreases suddenly.

There is a continuous addition of reactants.

The catalyst in the reaction becomes inactive.

Why does the addition of a catalyst increase the rate at which a reaction will occur?

It provides an alternative pathway with a lower activation energy.

It increases the temperature of the reaction.

It increases the concentration of reactants.

It absorbs excess heat from the reaction.

When you increase the temperature of a reaction, what happens to the rate at which it occurs? Why?

The rate increases due to increased molecular collisions.

The rate decreases because reactants are stabilized.

The rate decreases as reactants decompose.

The rate remains unchanged as temperature does not affect reactions.

When you decrease the surface area of a reaction, what happens to the rate at which it occurs? Why?

The rate decreases due to reduced contact between reactants.

The rate increases because there is less space for the reaction.

The rate increases as reactants are more concentrated.

The rate remains the same as surface area does not influence reaction rates.

What does a reversible reaction imply in chemical processes?

The reaction can proceed in both forward and reverse directions.

The reaction occurs only in one direction.

The reaction does not proceed to completion.

The reaction proceeds to completion without any reverse process.

What does a reversible reaction look like at dynamic equilibrium?

B) It looks like it has stopped.

A) It appears to be progressing.

C) It is only moving in one direction.

At equilibrium, how do the rates of the forward and reverse reactions compare?

C) The rates of the forward and reverse reactions are equal.

A) The rate of the forward reaction is higher.

B) The rate of the reverse reaction is higher.

D) The rates are unpredictable.

What happens to the concentration of the products and reactants at dynamic equilibrium?

D) The concentrations remain constant.

A) The concentrations steadily increase.

B) The concentrations steadily decrease.

C) The concentrations fluctuate widely.

What does Le Châtelier's Principle state about a system when it is stressed?

The system adjusts to retain equilibrium.

The system's equilibrium is permanently disrupted.

What happens to a chemical system when the concentration of a substance is increased?

The system shifts to decrease the concentration of that substance.

The system shifts to increase the concentration of that substance further.

The system shifts to produce heat.

What is the effect on a chemical system when there is a decrease in the concentration of a substance?

The system shifts to increase the concentration of that substance.

The system shifts to decrease the concentration of that substance further.

The system shifts to absorb more energy.

What happens to the concentrations of H₂ and N₂ when more N₂ is added to the system described in Le Châtelier's principle example for the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g)?

Both H₂ and N₂ concentrations decrease

Both H₂ and N₂ concentrations increase

H₂ concentration decreases and N₂ concentration increases

H₂ concentration increases and N₂ concentration decreases

What is the effect on the concentration of NH₃ when more N₂ is added to the system involving the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g)?

NH₃ concentration remains the same

NH₃ concentration first decreases then increases

According to Le Châtelier's Principle, what happens to the equilibrium when the concentration of SO2 is increased in the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g)?

The equilibrium shifts to the right

The equilibrium shifts to the left

The equilibrium remains unchanged

What is the effect of increasing the concentration of O2 in the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g)?

The equilibrium shifts to the right

The equilibrium shifts to the left

The equilibrium remains unchanged

If the concentration of SO3 is decreased in the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect on the equilibrium?

The equilibrium shifts to the left

The equilibrium shifts to the right

The equilibrium remains unchanged

What is the effect on the equilibrium when the concentration of a pure solid or liquid is changed in a reaction?

The equilibrium remains unchanged

The equilibrium shifts to the right

The equilibrium shifts to the left

According to Le Châtelier's Principle, what happens to the concentration of NaCl when the reaction 2Na(s) + Cl2(g) ⇌ 2NaCl(s) reaches equilibrium and no external changes are made?

The concentration of NaCl does not change

The concentration of NaCl increases

The concentration of NaCl decreases

The concentration of NaCl is zero

What happens to the direction of a chemical reaction when the temperature is increased in an exothermic reaction?

The reaction shifts towards the reactants.

The reaction shifts towards the products.

If ΔH is negative for a reaction, how is heat involved in the reaction?

Heat is absorbed from the surroundings.

Heat is neither absorbed nor released.

According to Le Châtelier's principle, if the temperature is increased for the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), in which direction will the equilibrium shift?

Reaction is unaffected by temperature changes

Is the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) endothermic or exothermic?

Both endothermic and exothermic

Neither endothermic nor exothermic

Match the following Reaction Rate affect with the definition of why it speeds up reactions.

The higher of this, the smaller of the volume, causing more particle collisions

This substance speeds the reaction rate by lowering the activation energy needed to start the reactions

The more of this causes there to be more room for the particles to collide and react with one another

Higher amounts of this of this leads to more frequent collisions between reactant particles

The higher the ______, the faster the reaction because more particles are moving and colliding, thus contacting with each other to react.

Unit 11 Review

Authored by Alyssa Harris

Chemistry

10th Grade

NGSS covered

Used 2+ times

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48 questions

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the minimum energy required for a chemical reaction to proceed called?

Reaction energy

Activation energy

Kinetic energy

Potential energy

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the term for the point in a chemical reaction where old bonds begin breaking and new bonds start forming?

Reaction intermediate

Transition state

Activated complex

Catalyst point

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the role of a catalyst in a chemical reaction?

To consume the reactants

To produce the products

To increase the reaction temperature

To lower the activation energy

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the term used to describe the speed of a chemical reaction?

Reaction time

Reaction rate

Reaction speed

Reaction interval

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following reactions would typically occur at the fastest rate?

Digesting food

Combusting gasoline

Converting graphite to diamond

Lighting a match

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

On a scale from 1 to 3, where 1 is the slowest, how would you rate the reaction rate of converting graphite to diamond?

Not applicable

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the rate of a chemical reaction expressed as?

The amount of product formed per unit time

The amount of reactant changing per unit time

The speed of product decomposition

The time it takes for a reaction to complete

Tags

NGSS.HS-PS1-5

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Unit 11 Review

What is the minimum energy required for a chemical reaction to proceed called?

What is the term for the point in a chemical reaction where old bonds begin breaking and new bonds start forming?

What is the role of a catalyst in a chemical reaction?

What is the term used to describe the speed of a chemical reaction?

Which of the following reactions would typically occur at the fastest rate?

On a scale from 1 to 3, where 1 is the slowest, how would you rate the reaction rate of converting graphite to diamond?

What is the rate of a chemical reaction expressed as?

Which of the following is an example of a very fast reaction?

What type of reaction speed is associated with the setting of concrete?

Which factor increases the rate of a chemical reaction by providing an alternative pathway with a lower activation energy?

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