Rates of reaction

Question 1

How can we show the rate of a reaction?

Answer 1

Use a graph with amount of product formed on the y axis and time on the x
Alternatively, the graph has reactant used on y axis instead

Question 2

On a graph with amount of product formed, what shape is the curve and why?

Answer 2

Curve is upwards
Because the reactant molecules become the product molecules thus increase in product formed

Question 3

On a graph with amount of reactant used, what shape is the curve and why?

Answer 3

Curve is downwards
Because the reactant molecules form product molecules thus there’s a decrease in reactant

Question 4

On these graphs, what does the curve and its gradient show?

Answer 4

The rate of reaction at that specific point

Question 5

On a product formed graph, what structure does the curve usually follow and why?

Answer 5

Begins increasing rapidly = product formed quickly = more collisions = more reactant particles to collide
Flattens out because less reactant particles = less collisions = less product made

Question 6

On a reactant used graph, what structure does the graph usually follow and why?

Answer 6

Rapid decreasing = the most number of reactant particles = more collisions = more product being made so less particles all together
Flattens because less reactant particles = less collisions = less reactant used

Question 7

When does a reaction stop?

Answer 7

No more reactant molecules

Question 8

What do you measure a solid product in?

Answer 8

grams (g)

Question 9

What do you measure a gas product in?

Answer 9

Cm3

Question 10

Mean rate of reaction

Answer 10

Average rate of reaction over the whole reaction

Question 11

How to find the mean rate of reaction?

Answer 11

Amount of product formed/ reactant used
———————————————
Total time taken of reaction

Question 12

What is the rate of reaction measured in?

Answer 12

g/s or cm3/s

Question 13

What is important about the mean rate when calculating it?

Answer 13

You do not need to use a graph, just the total amount divided by the total time

Question 14

What do you need when calculating the rate at a specific point?

Answer 14

A tangent on the graph!!!

Question 15

Why do you need to draw a tangent to find rate at a specific point?

Answer 15

Because the curve constantly changes, so does the rate
So you must estimate it with a tangent

Question 16

How to draw a tangent to find the rate of reaction at a specific point?

Answer 16

Go to the specific time it asks for
Find that point on the curve and draw a tangent to it
Connect the 2 ends of the tangent to make triangle
Find the difference between x and y values Of the triangle
y/x = estimated rate of reaction

Question 17

What effects the rate of a reaction?

Answer 17

Concentration
Surface area
Temperature
Catalysts used

Question 18

Concentration

Answer 18

The amount of specific particles in a given volume

Question 19

Collision theory

Answer 19

Reactions happen when reacting particles collide with sufficient energy
Therefore the rate of reaction = amount of times there’s a successful collision thus reaction happens faster

Question 20

How does a higher concentration affect the ROR?

Answer 20

High concentration of particles = more successful collisions = collisions per second increases = higher rate of reaction

Question 21

How does a lower concentration affect the ROR?

Answer 21

Low concentration of particles = less successful collisions = collisions per sec decreases = lower rate of reaction

Question 22

How does the concentration correlate to the shape of the curve on a graph?

Answer 22

On a product formed graph, as this begins with lots of reactant to none
Rapid incline at first because higher concentration of reactant particles = more collisions = more product formed
Flattens = lower concentration of reactant particles = less collisions = less product formed
Flat at the end = no reactant particles = no collisions

Question 23

How does the effect of concentration apply to reacting gases?

Answer 23

More molecules = more collisions has the same effect
Although in this case it is not the concentration but the pressure

Question 24

What does the rate if reaction depend on?

Answer 24

The number of successful collisions per second

Question 25

If we have higher concentration of reactant molecules, how does this effect the reaction compared to if we had lower?

Answer 25

When it is higher concentration, the rate of reaction is increased because there are more particles so more successful collisions per second Also more product is formed because we had more reactant molecules at the start anyway

Question 26

When does the surface area effect the rate of reaction?

Answer 26

When a solid is reacting with a liquid or gas

Question 27

How does surface area effect rate of reaction?

Answer 27

In a solid, particles on the surface of the solid can only react with the liquid/gas particles and not the underlying layers Therefore a larger surface area = more exposed particles = more collisions per second = increased rate of reaction

Question 28

What experiment shows how surface area effects rate of reaction?

Answer 28

Conical flask with hydrochloric acid Place marble powder inside Connect flask to a bung and delivery tube Put measuring cylinder with water in a water tray above delivery tube Measure how long it takes for marble to produce carbon dioxide Calculate rate of reaction with amount produced/ time Repeat with different sized marble samples and compare

Question 29

How can we find a more accurate reading of carbon dioxide produced when measuring effect of surface area?

Answer 29

Gas syringe

Question 30

How else can we measure effect of surface area on rate of reaction?

Answer 30

Find the amount of carbon dioxide lost when marble reacts with HCl Place conical flask with marble chips in hydrochloric acid on a balance Block top of flask with cotton wool Cotton wool let’s co2 out put prevents acid leaving Therefore gives us an accurate result

Question 31

Collision theory

Answer 31

Chemical reactions can only take place when reacting particles collide with each other The collisions must have sufficient energy therefore be successful collisions Rate of reaction depends upon amount of successful collisions per second

Question 32

Activation energy

Answer 32

Minimum amount of energy the particles must have to collide successfully And therefore react

Question 33

How does temperature effect the rate of reaction?

Answer 33

Increasing temperature = increases energy of particles = move faster, colliding more times per second = increase rate of reaction Also have more energy to overcome activation energy battier thus collide successfully

Question 34

Catalysts

Answer 34

Increase rate of reaction so they are quicker Are not used up in the reaction Useful as when using them you don’t have to increase temp, saving money Also because they are reusable

Question 35

How do catalysts affect rate of reaction

Answer 35

They increase it Because they provide a different pathway for the reaction That has lower activation energy Therefore more reacting particles can cross this activation energy barrier = more successful collisions

Question 36

Do we include catalysts in a word chemical equation?

Answer 36

No they aren’t because they don’t get used up

Question 37

Can we use the same catalyst for all reactions?

Answer 37

No different reactions require different catalysts