Rates of reaction Flashcards
1
Q
Define rate of chemical reaction
A
- How fast the reactants are changed into products
2
Q
Example of fast reactions
A
- Burning is a fast reaction
- Explosions are a faster reaction and release a lot of gas and there over in a fraction of a second
3
Q
Example of slow reactions
A
- Rusting of iron
- reactions which include chemical weathering
4
Q
Example of moderate speed reaction
A
- metal mg reacting with acid to produce gentle stream of bubbles
5
Q
The —– the line on the graph, the ——- the reaction
A
steeper, faster
6
Q
What do the fastest reactions have?
A
a steeper gradient at the beginning and become horizontal sooner than slower reactions.
7
Q
Define the collision theory
A
- chemical reactions occur only when the reactant particles collide with sufficient energy to react. The minimum amount of energy needed is called the activation energy.
8
Q
What do the chemical reactions depend on?
A
1) The collision frequency of reacting particles. The more collisions, the faster the reaction.
2) The energy transferred during a reaction. Particles have to collide with enough energy for the collision to be successful.
9
Q
What does the rate of reaction depend on?
A
- Temperature
- Surface area
- Presence of a catalyst
- The concentration of a solution or the pressure of a gas.
10
Q
more —– increase the rate of reaction
A
- collisions
- It increases the number of successful collisions between the reacting particles
11
Q
A
