Year 10 – ChemistryRates of Reactions

Week starting 6th April

Revision Guide

Rates of Reactions – Topic C6 – Page 142 → 149

Rates of reactions

Factors affecting rates of reactions

Measuring rates of reactions

Two rates experiments

Finding reaction rates from graphs

Reversible reactions

Le Chatelier’s Principle

HIGHER AND SEPARATES ONLY!!

Rates of Reactions – Topic C6 Page 142 → 149

Rates of reactions https://www.youtube.com/watch?v=eSInI1xHvh4&t=38shttps://www.youtube.com/watch?v=OttRV5ykP7A

Factors affecting rates of reactions https://www.youtube.com/watch?v=u4Co4N-Jmbshttps://www.youtube.com/watch?v=WojotwxPD6I&list=PL9IouNCPbCxW8AN0t0py7LaKdKSwfL3fP&index=5https://www.youtube.com/watch?v=G2TEfhwgq84&list=PL9IouNCPbCxW8AN0t0py7LaKdKSwfL3fP&index=6https://www.youtube.com/watch?v=hel8fQjxcO8&list=PL9IouNCPbCxW8AN0t0py7LaKdKSwfL3fP&index=7

Measuring rates of reactions https://www.youtube.com/watch?v=Gl6LVl7oAlU

Two rates experiments https://www.youtube.com/watch?v=ssa3wh3RNt0https://www.youtube.com/watch?v=0RUYNpdnALg

Finding reaction rates from graphs https://www.youtube.com/watch?v=UkrBJ6-uGFAhttps://www.youtube.com/watch?v=6LV63WtuvJg

Reversible reactions https://www.youtube.com/watch?v=66qcNNJFy6E&list=PL9IouNCPbCxW8AN0t0py7LaKdKSwfL3fP&index=8

Le Chatelier’s Principle https://www.youtube.com/watch?v=utmV4Q0t6MI&list=PL9IouNCPbCxW8AN0t0py7LaKdKSwfL3fP&index=9https://www.youtube.com/watch?v=SlI5m0RQqik&list=PL9IouNCPbCxW8AN0t0py7LaKdKSwfL3fP&index=10https://www.youtube.com/watch?v=hngzmRrAXTE&list=PL9IouNCPbCxW8AN0t0py7LaKdKSwfL3fP&index=11

On-line learning clips

Required Practical's https://www.youtube.com/watch?v=N5p06i9ilmo&list=PL9IouNCPbCxW8AN0t0py7LaKdKSwfL3fP&index=4

HIGHER AND SEPARATES ONLY!!

TASK 1 – Time 2 → 3hrs

Here are some simple mind maps that I have done, can you add extra concepts to them?

You could do this by using your revision guide or watching the clips I have found for you.

You could print out and add OR do your own in your book or on paper.

HIGHER AND SEPARATES ONLY!!

TASK 2 - Time 1hr

In this topic there is 1 Required Practical, Rates of Reaction.

Here is a sheet to summaries these required practical’s, ADD details to complete them.

You could do this by using your revision guide or watching the clips I have found.

You could print out and add Or do your own in your book or on paper.

Required Practicals: Chemistry

Rates of Reaction – Note there a three ways in which you can measure the rate of reaction: Precipitation, Mass change or Volume of gas given off.

Variables

Method

Keywords Other types of question

TASK 3 – Time 1 hr

Mini Quiz

Have a go at the quiz and mark it using the mark scheme.

Ensure you check each page of questions as there are some just for Separates and Higher.

You could print the quiz out OR complete it in your book or on paper.

Quiz – Rates of Reactions

Quiz 1:

1. State 2 formulae used to calculate rate of reaction (2 marks)

2. State 2 units (3 for Higher & Separate science) for quantity of reactant (2 marks).

3. State 2 units of rate of reaction (2 marks).

4. Describe how the rate of reaction can be measured using an inverted measuring cylinder and a delivery tube in water.

5. Describe how the rate of reaction can be measured using a gas syringe.

6. Describe how the rate of reaction can be measured using a balance.

7. Describe how the rate of reaction can be measured using the colour change.

Quiz 1 (Answers)

1. Quantity of reactant used or Quantity of product formed

time time

2. cm3, g, moles.

3. Cm3/s, g/s, mol/s

4. Fill a measuring cylinder and large tub with water. Turn the measuring cylinder upside down in the water and secure upright. Connect the delivery tube to the reaction vessel (e.g. conical flask) and place the other end into the measuring cylinder through water. As gas is produced, the water will be displaced and volume can be read from the cylinder.

5. Connect a gas syringe to the reaction vessel using a delivery tube. As gas is produced the plunger on syringe will move. At the end of the reaction, record the volume of gas inside the syringe.

6. Add reactants to a flask and quickly place cotton wall in the flasks neck. Place onto a balance and record the starting mass. At the end of experiment record the new mass and calculate the difference. This value is the mass of gas produced.

7. Add the reactants to a flask. Place a large, dark mark on some paper underneath the flask. As the solution changes colour the mark will become more difficult to see. Record the time taken for this to be no longer visible.

Quiz 2

1. For chemical reactions to occur, the particles must _________ with each other and with sufficient __________. (2 marks)

2. What is the minimum amount of energy required to react called?

3. State the 4 factors that can increase the rate of reaction (4 marks)

4. Explain how a catalyst affects the rate of reaction (2 marks).

5. Name a biological catalyst.

1. Collide, Energy

2. Activation energy

3. Concentration or pressure, surface area, temperature, using a catalyst

4. Catalysts increase the rate of reaction. They work by providing an alternative reaction pathway with a lower activation energy.

5. Enzymes such as lipase are biological catalysts.

Quiz 2 (Answers)

Quiz 3

1. Explain how a catalyst affects the rate of reaction (2 marks).2. Name a biological catalyst.3. What is a reversible reaction?4. Which symbol is used instead of an arrow in a reversible reaction?5. If a reversible reaction is exothermic in one direction, it is

_______________________ in the other.6. In a reversible reaction, the ________ _________ of energy is transferred

in each direction.7. What is equilibrium?8. How can equilibrium be reached?9. Give an example of a reversible reaction.

1. Catalysts increase the rate of reaction. They work by providing an alternative reaction pathway with a lower activation energy.

2. Enzymes 3. The products in a reversible reaction can react to form the reactants

again. 4. ⇌5. Endothermic6. Same rate7. Equilibrium is when both reactions are still happening but there is no

overall effect.8. In a closed system.9. Hydrated copper sulphate ⇌ Anhydrous copper sulphate + Water

Quiz 3 (Answers)

Quiz 4 Higher & Separate only

1. Whose principle is used to explain equilibrium?

2. If the concentration of one of the reactants or products is changed, the system is no longer at _______________.

3. If the concentration of a reactant is increased, _______ products will be formed until equilibrium is reached again.

4. If the concentration of a product is decreased, _______ reactants will be formed until equilibrium is reached again.

For gaseous reactions at equilibrium:

5. An increase in pressure causes the equilibrium position to shift towards the side with the ___________ number of molecules as shown by the symbol equation for that reaction

6. A decrease in pressure causes the equilibrium position to shift towards the side with the __________ number of molecules as shown by the symbol equation for that reaction.

If the temperature of a system at equilibrium is increased:

7. The relative amount of products at equilibrium _____________ for an endothermic reaction

8. The relative amount of products at equilibrium ______________ for an exothermic reaction.

If the temperature of a system at equilibrium is decreased:

9. The relative amount of products at equilibrium ______________ for an endothermic reaction

10. The relative amount of products at equilibrium ______________ for an exothermic reaction.

1. Le Chatelier2. Equilibrium3. More 4. Less5. Fewer6. Greater7. Increase8. Decrease9. Decrease10. Increase

Quiz 4 Higher & Separate only (Answers)

Task 4 – Reflection – Time 30 mins

After you have completed the quiz, have you identified any gaps in your mind maps?

If so, add to your mind map (Task 1 and 2)

Reflection – Complete the table so you know where you need to focus extra revision on.

Topic How confident are you after completing

the set tasks? (1 → 10 ☺ )

Areas that you still need to focus on?

Questions to ask your teacher?

Rates of reactions

Factors affecting rates of reactions

Measuring rates of reactions

Two rates experiments

Finding reaction rates from graphs

Reversible reactions

Le Chatelier’s Principle

HIGHER AND SEPARATES ONLY!!