Kinetics Flashcards
What must happen for a reaction to occur?
Particles must collide.
What is the rate of reaction?
The change in concentration or amounr of a reactant or product per unit time.
What is the equation or rate?
Amoutn of reactant used or product made divided by time.
What does the collision theory state?
For a reaction to occur the particles must collide in the right direction / orientation and they must have a minimum amount of kinetic energy.
What is the activation energy?
The minimum amount of energy required for a reaction to occur.
What does the maxwell-boltzmann distribustion show?
The energy in gas particles.
Where does the maxwell-boltzmann distribution curve start?
At 0,0 as none of the particles have zero kinetic energy.
What does the area under the maxwell-boltzmann distribution represent?
The total number of molecules.
How does increasing the temperature affect the maxwell-boltzmann distribution curve?
The curve shifts to the right as a larger proportion of the molecules will have energy greater than the activation energy. The peak is lower.
How does decreasing the temperature affect the maxwell-boltzmann distribution curve?
The curve shifts to the left as a smaller proportion of molecules will have energy greater than the activation energy. The peak will also be higher.
Why do we get a faster rate of reaction when temperature is increased?
The particles move around more at higher temperatures meaning that they will collide more often and hence the rate of reaction will increase.
Why do small increases in temperature lead to a large increase in rate?
Due to the combination of more collision and more energetic collisons.
How does introducing a catalyst affect the maxwell-boltzmann distribution curve?
The curve stays the same however the activation energy lowers and shifts to the left so more particles have the energy to react.
