The rate of reaction depends on
Frequency of collisions between particles and energy of their collisions
Frequency of moving electrons
Amount of reactants used
How do you calculate rates of reactions?
time taken for change /change in reactant or product (x/y)
change in reactant or product/ time taken for change (y/x)
A factor affecting the rate of reaction is increased temperature.
Factors affecting the rate of reaction include
state, temperature and surface area, use of catalyst
volume of reactant, pressure and temperature, use of catalyst
temperature,concentration or pressure, surface area, use of catalyst
At a ❌ concentration, there is ❌ particles in the same amount of space. This means the particles are more likely to collide and therefore more likely to ❌
As the pressure increases, the space in which the gas particles are moving becomes
smaller
bigger
The gas particles become closer together as the pressure increases causing less frequent collisions. This means the particles are less likely to react.
Catalysts are substances that increase the rate of reaction without being used up in the reaction. Catalysts never produce more product - they just produce the same amount of energy more quickly.
Catalysts work by
increasing activation energy
decreasing activation energy
Catalysts are important to industry because
Products can be made slower, reduce the need for higher temperatures and they can be reused
Products can be made quicker, reduce the need for higher temperature and they can't be reused
products can be made quicker, reduce the need for higher temperature and they can be reused
products can be made quicker, increase need for higher temperature and they can be reused
Any reaction involving a solid can only take place at the surface of the solid. If the solid is spilt into several pieces, the surface area ❌. This means that there is an ❌ area for the reactant particles to collide with. The smaller the pieces, the ❌ the surface area. This means ❌ collisions and a ❌ chance of reaction.
At a ❌ temperature, particles have ❌ energy. This means they move ❌ and are more likely to collide with other particles. Also when the particles do collide they do so with more energy and so the number of successful collisions ❌
