Kinetics Flashcards
What is the collision theory?
A reaction only happens when particles collide with enough energy.
What is the activation energy?
The minimum amount of energy particles need to collide with for a reaction to occur.
Draw the Maxwell-Boltzmann distribution?
Why does the curve start at the origin?
Why is the mean energy to the right of the most probable energy?
Draw how the curve is affected by higher and lower temperatures.
What effect does an increase in temperature have on the rate of reaction?
The particles have more kinetic energy meaning that more particles will have an energy that is bigger than the activation energy. This means there will be more frequent and successful collisions.
Draw how the curve is affected by a lower and higher concentration.
What effect does an increase in concentration have on the rate of reaction?
There will be more particles per unit of volume meaning that there will be more particles that have an energy that is higher than the activation energy. This means there will be more frequent and successful collisions.
What are catalysts?
They speed up a reaction without being used up.
How do catalysts increase the rate of reaction?
They provide an alternative reaction pathway which lowers the activation energy.
How does the use of a catalyst affect the Maxwell-Boltzmann curve?
What is the rate of reaction?
The change in the amount of product or reactant per unit of time.
What are the ways for measuring the rate of reaction?
- Measuring how long it takes for a precipitate to form.
- Measuring the change in mass.
- Collecting gas produced in a gas syringe.
