Rates & Extent Of Reactions

Question 1

What is an anomalous result?

Answer 1

Result that doesn’t fit in with the pattern of the other results.

Question 2

Anomalous results can be easily ________ in the data and ____________,

Leading to a more _________ calculation of the mean.

Answer 2

Spotted
Discarded

Accurate

Question 3

What is rate of reaction

Answer 3

The speed at which a product is formed or reactant is used up.

Question 4

How can the rate reaction be sped up/increased

Answer 4

Increased temperature

Increased concentration

Increased surface area

Increased pressure

Use a catalyst

Question 5

What are the equations for rate of reaction?

Answer 5

Rate of reaction = mass or volume of product formed / time

Rate of reaction = mass or volume of reactants lost / time

In simple terms it’s volume / time

Question 6

What are the units for rate of reaction?

Answer 6

g/s

cm^3/s

Question 7

What is needed for a chemical reaction to happen

Answer 7

Reactant particles must collide with each other

The particles must have ENOUGH activation energy for them to react

Question 8

If particles collide with out enough activation ________ the particles just ________ off each other.

Answer 8

Energy

Bounce

Question 9

How does temperature affect the rate of reaction?

Answer 9

Increases the particles energy (activation),

which increases the number of successful collisions;

which means collisions are more frequent,

this finally increases the rate of reaction.

Question 10

What is a control variable

Answer 10

What you keep the same

Question 11

What is the independent variable

Answer 11

What you change

Question 12

What is the dependent variable

Answer 12

What you measure

Question 13

What is the concentration of a solution?

Answer 13

A measure of the number of particles in a certain amount of space

Question 14

Collision theory + concentration:

Increasing concentration means there are _______ particles in the ______ amount of space.

So more ________ collisions.

Thus an _________ in the rate of reaction.

Answer 14

More
Same

Successful

Increase

Question 15

Disappearing cross RP

1. Using a measuring ________, add __cm^3 of dilute solution t___________ solution to a conical _______.

Answer 15

Cylinder
50
Thiosulfate
Flask

Question 16

Disappearing cross RP

2. Place a conical ______ on a piece of ______ with a black _______ drawn on it.

Answer 16

Flask
Paper
Cross

Question 17

Disappearing cross RP

3. Using a different measuring ________, add __cm^3 of dilute h___________ acid to the conical flask. Immediately swirl the flask to mix it’s contents and start a ________.

Answer 17

Cylinder
10
Hydrochloric
Stopwatch

Question 18

Disappearing cross RP

4. M_______ and r________ the temperature of the reaction mixture.

Answer 18

Measure and record

Question 19

Disappearing cross RP

5. _______ down through the reaction mixture. When the cross is no longer __________, record the ____ on the stopwatch.

Answer 19

Look
Visible
Time

Question 20

Disappearing cross RP

6. Measure and record the t_________ of the reaction mixture, and clean the apparatus.
7. Realest steps _____ with different s_____ temperatures of sodium t_______ solution.

Answer 20

Temperature

1-6
Starting
Thiosulfate

Question 21

As you increase the concentration of sodium thiosulfate the rate of reaction ___________.

This is because as there are _____ particles in a set amount of space, there are more _______/successful collisions.

Answer 21

Increases

More
Frequent

Question 22

How can you describe the relationship of a graph?

Answer 22

Is it linear (straight line graph)
Is it non-linear (curved graph)

“The rate of —— increases as —— increases”

Quote value descriptions (numbers)

Question 23

What equipment do you use in the process of collecting a gas?

Answer 23

Beehive 
Delivery tube 
Water tough 
Clamp 
Measuring cylinder 
Water 
Dilute acid 
Magnesium ribbon

Question 24

Describe the process of collecting a gas

Answer 24

Set up equipment.

Add Mg to the 30ml of 1M HCI.

Every 10 seconds record how much gas is produced.

Record your results in your table.

Repeat at different concentration.

The higher concentration of acid, rate of reaction increases.

Question 25

Describe and explain how surface area changes the rate of reaction

in terms of particles and collisions

Answer 25

If the surface area of a reactant is increased:

• More particles are exposed to the other reactant.
• There are more collisions.
• The rate of reaction increases.

Question 26

Rate = y/x

Gradient of tangents to calculate rate of reaction

Answer 26

You’re welcome for the free answer lols.

Question 27

Describe and explain how pressure changed the rate of reaction

in terms of particles and collisions

Answer 27

The greater the frequency of successful collisions, the greater the rate of reaction.

If the pressure of a reacting gas is increased:

• the reactant particles become more crowded
• the frequency of collisions between reactant particles increases
• the rate of reaction increases

Question 28

A catalyst is a substance that _______ up a reaction without being _____ up in the reaction itself.

This means that it’s not part of the ______ reaction equation.

Answer 28

Speeds
Used

Overall

Question 29

Different catalysts are needed for ________ reactions, but they all work by __________ the activation energy needed for the reaction to occur.

They do this by providing an alternative reaction __________ with a _______ activation energy.

Answer 29

Different
Decreasing

Pathway
Lower

Question 30

Enzymes are biological c_________ - they c________ reactions in living things.

Answer 30

Catalysts

Catalyse

Question 31

What is a reaction profile?

Answer 31

A diagram showing the change in chemical particle energy,

referred to as the energy pathway,

as a chemical reaction proceeds from reactants to products.