Free Printable Rates of reaction/Le Chateliers

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Rates of reaction/Le Chateliers

Total questions: 22

Worksheet time: 19mins

Name

Class

Date

2SO_2(g)+O_2(g)⇌ 2SO_3(g) + Heat

Adding SO_2(g)will

shift equilibrium right

shift equilibrium left

increase rate of reaction

have no change

2SO₂(g)+O₂(g) ⇌ 2SO₃(g) + Heat

Increasing the temperature will...

shift equilibrium right

shift equilibrium left

increase pressure

have no change

2SO_2(g) + O_2(g) ⇌ 2SO_3(g)+ Heat

Removing O_2(g) will

shift equilibrium right

shift equilibrium left

increase pressure

have no change

2SO₂(g)+1O₂(g) ⇌ 2SO₃(g) + Heat

Increasing the pressure on the system will...

shift equilibrium right

shift equilibrium left

slow rate of reaction

have no change

2CrO₄^2- + 2H⁺ → Cr₂O₇^2- + H₂O

What will happen when H⁺ ions are added to the system?

Position of equilibrium will shift to left and become more yellow

Color of system will turn all yellow

Color of system will turn all orange

Equilibrium will shift to right and become more orange

Increase in temperature of the reactants can do one of the following

Slow collision frequency

Allow less effective collision between the particles

Neutralise the reaction

increase collision between the particles thus increasing the rate.

Why does a catalyst increase the rate of reaction?

it produces extra energy for the reactants

it increases the speed of the reactant particles

it increases the frequency of particle collisions

it reduces the activation energy of the reaction

Which of the following increase the reaction rate?

less surface area

lower temperature

an inhibitor

increased concentration

Why don't all collisions between particles cause a reaction?

the particles also need to collide with a catalyst

not all the particles collide with enough energy

not all the particles collide at a high enough temperature

the particles need to collide with each other twice

10.

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

Place the reactants in hot water

Place the products in ice bath

Place the reactants in a ice bath

Keep stirring the reactants with a stirring rod

11.

How could we make this reaction happen more quickly?

Decrease the concentration of the acid

crush the chalk to increase the surface area

Put the test tube in an ice bath

12.

ΔH value in an endothermic reaction is a positive number.

True

False

13.

What is the Heat of Reaction $\Delta H$ for this reaction?

-200 KJ

200 KJ

400 KJ

-300 KJ

14.

How much activation energy is needed for this reaction?

300 KJ

500 KJ

400 KJ

100 KJ

15.

Are the products or reactants of this reaction storing more energy in their chemical bonds?

Both storing the same

No way to tell

Products

Reactants

16.

What type of reaction is this?

Exothermic

Endothermic

Energy Producing

No way to tell

17.

What kind of equation is this: 2KI + MgCl₂ + 200KJ ----> 2KCl + MgI₂

Endothermic

Exothermic

18.

How can you tell this reaction is exothermic: MgO + CaS ----> CaO + MgS + 200 KJ

Energy is written on the products side

Energy is being released

Less energy is stored on product side

All of these tell me

19.

During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______.

Warm

Cold

20.

What is the ΔH of this reaction?

40 kJ

20 kJ

80 kJ

-60 kJ

21.

What is the energy of the activated complex?

75 kJ

225 kJ

300 kJ

225 kJ

22.

What is the PE of the products?

100 kJ

175 kJ

50 kJ

75 kJ

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Rates of reaction/Le Chateliers

Total questions: 22

Worksheet time: 19mins

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