Chem -6 Flashcards
What is rate of reaction
A measure of how quickly a reactant is used up or a product is formed
What is needed for a chemical reaction to happen
Reactant particle must collide together
And the particles must have enough energy to react
What is activation energy
The minimum amount of energy needed for a collision to be successful
What happens to catalyst at the end of a reaction
Nothing
What will increase the proportion of successful collisions
Increasing the temperature and surface area
Would would speed up a reaction
Pressure , concentration or catalyst
What is a reversible reaction
The products of the reaction can react together to produce the original reactants
How can the position is equilibrium be changed (le chateliers principle)
Change in pressure, concentration and temperature
What has the smallest surface area to volume ratio
Large lumps
What happens if a large lumps is divided or ground into powder
-total volume stays the same
-area of exposed surface increases
- the surface area to volume ratio increases
What is better at increasing frequency of successful collisions and why
(Lumps or powders)
Powders because they have a higher surface area to volume ratio so
-more reactant particles are exposed at the surface
-the frequency of successful collisions are increased
- rate of reaction increases
How do catalyst increase rate of reaction
Provide alternative pathway with lower activation energy
How does temp, pressure, concentration and surface area increase rate of reaction and successful collision rate
They increase the frequency of particles colliding their for more chance of the collisions being successful and speeding up a reaction