Collision theory states that:

atoms, ions, and molecules must collide with enough energy to react

atoms, ions, and molecules must collide to react

atoms, ions, and molecules must have enough energy to react

atoms, ions, and molecules can react at any time, doesn't matter how close they are or how much energy they have.

How do catalysts work to affect rate of reaction?

They lower the activation energy of the reaction

They increase the energy of the reactants

They increase the number of collisions

They increase the activation energy of the reaction

A reversible reaction is at equilibrium. This means that _______.

The forwards and backwards reactions are happening at the same rate

There are equal amounts of reactants and products

The reaction has now completely stopped

In a reversible reaction, if the forwards reaction is exergonic then the backwards reaction is _____.

we can't tell from this information

A reversible reaction is at equilibrium. The temperature of the reaction is increased. How will the equilibrium shift?

The endothermic reaction will speed up

The exothermic reaction will speed up

Consider the following reaction: N 2 O 4 (g) $$\leftrightarrow$$ 2NO 2 (g). If we increase the pressure on the reaction, which way will the equilibrium shift?

To the left, as this will decrease the number of molecules of gas and reduce pressure.

To the right, as this will decrease the number of molecules of gas and reduce pressure.

To the left, as this will increase the number of molecules of gas and increase pressure.

To the right, as this will increase the number of molecules of gas and increase pressure.

Consider the Haber process shown here. If we increase the temperature of the reaction, what will happen to the equilibrium?

It will move to the left and produce more H 2 and N 2

It will move to the right and produce more ammonia (NH 3 )

It will move to the left and produce more ammonia (NH 3 )

It will move to the right and produce more H 2 and N 2

Le Chatelier's principle states that if we change the conditions of a reversible reaction, ________________.

The equilibrium will shift to oppose that change

The equilibrium will shift to increase that change

The equilibrium will not change

Consider this reversible reaction at equilibrium. If you increase the concentration of C and D, what will happen to the equilibrium?

It will shift to the left to produce more A and B

It will shift to the right to produce more C and D

We need more information to answer this

Reaction Rates and Equilibrium

Quiz

•

Chemistry

•

8th Grade

•

Practice Problem

•

Hard

•

NGSS

HS-PS1-5, HS-PS1-6

Standards-aligned

Charles Martinez

Used 1+ times

FREE Resource

6.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

HCl is reacted with Zn to form ZnCl₂ and H₂ gas. The concentration of HCl is increased from 0.5 mol/L to 2 mol/L. What happens to the rate of reaction?

It will increase

It will stay the same

It will decrease

Tags

NGSS.HS-PS1-5

7.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

A reaction mixture of NaOH and formaldehyde is cooled from 80^oC to 0^oC. What happens to the rate of reaction?

It will increase

It will stay the same

It will decrease

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Reaction Rates and Equilibrium

21 questions

An increase in temperature will cause:

An increase in volume of gases will cause:

An increase in pressure of gases will cause:

An increase in concentration of a solution will cause:

An increase in surface area of reactants will cause:

HCl is reacted with Zn to form ZnCl₂ and H₂ gas. The concentration of HCl is increased from 0.5 mol/L to 2 mol/L. What happens to the rate of reaction?

A reaction mixture of NaOH and formaldehyde is cooled from 80^oC to 0^oC. What happens to the rate of reaction?

H₂ gas and O₂ gas are reacting together to form water in a sealed container. The volume of the container is expanded from 2L to 10L. What will happen to the rate of reaction?

Magnesium can combust in air to form magnesium oxide. If we use a fine powder of Mg instead of a solid block, what will happen to the rate of reaction?

The Haber process reacts together H₂ and N₂ gases to form NH₃. What will happen to the rate of reaction if we increase the pressure of these gases?

Create a free account and access millions of resources

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

Reaction Rates and Equilibrium

21 questions

An increase in temperature will cause:

An increase in volume of gases will cause:

An increase in pressure of gases will cause:

An increase in concentration of a solution will cause:

An increase in surface area of reactants will cause:

HCl is reacted with Zn to form ZnCl2 and H2 gas. The concentration of HCl is increased from 0.5 mol/L to 2 mol/L. What happens to the rate of reaction?

A reaction mixture of NaOH and formaldehyde is cooled from 80oC to 0oC. What happens to the rate of reaction?

H2 gas and O2 gas are reacting together to form water in a sealed container. The volume of the container is expanded from 2L to 10L. What will happen to the rate of reaction?

Magnesium can combust in air to form magnesium oxide. If we use a fine powder of Mg instead of a solid block, what will happen to the rate of reaction?

The Haber process reacts together H2 and N2 gases to form NH3. What will happen to the rate of reaction if we increase the pressure of these gases?

Create a free account and access millions of resources

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

HCl is reacted with Zn to form ZnCl₂ and H₂ gas. The concentration of HCl is increased from 0.5 mol/L to 2 mol/L. What happens to the rate of reaction?

A reaction mixture of NaOH and formaldehyde is cooled from 80^oC to 0^oC. What happens to the rate of reaction?

H₂ gas and O₂ gas are reacting together to form water in a sealed container. The volume of the container is expanded from 2L to 10L. What will happen to the rate of reaction?

The Haber process reacts together H₂ and N₂ gases to form NH₃. What will happen to the rate of reaction if we increase the pressure of these gases?