2.4 - Rates Of Reaction Flashcards Preview

AQA GCSE - Chemistry > 2.4 - Rates Of Reaction > Flashcards

Flashcards in 2.4 - Rates Of Reaction Deck (12)
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1
Q

What is the rate of reaction?

A

How quickly all reactants are used up
Or
A measurement of how quickly new products are made

2
Q

What is the Collision Theory

A

The particles of the reactants need to collide having frequent successful collisions above the activation energy

3
Q

What is the activation energy?

A

The minimum amount if energy particles must have to react

4
Q

How does temperature effect the rate of reaction

A

It gives the particles more kinetic energy. The vibrate and move more at a greater force causing more frequent collisions above the activation energy. Increasing the rate of reaction

5
Q

How does concentration effect the rate of reaction

A

Higher concentration means there are more particles therefore more opportunities for successful frequent collisions. This will increase the rate of reaction

6
Q

How will surface area effect the rate of reaction?

A

A higher surface area means there are more particles exposed to the acid so there are more successful frequent collisions above the activation energy. This will increase the rate of reaction

7
Q

Which has a higher surface area? Marble chips or Marble powder

A

Marble powder

8
Q

What does a catalyst do?

A

It lowers the activation energy. Allowing more successful frequent collisions above the activation energy

9
Q

Are catalysts used up in a reaction? How can you tell?

A

No, they have the same mass at the start and end of the reaction

10
Q

Do all reactions use the same catalyst?

A

No

11
Q

Why are catalysts important in industrial processes?

A

To reduce the energy which will reduce the costs and environmental impact

12
Q

Are catalysts costly? Economical?

A

Expensive but economical as they don’t need replacing often