Kinetics Flashcards
(13 cards)
1
Q
What is rate of reaction? (2)
A
- The change of amount of
reactant of product per time (1)
Rate = Amount of reactant / Time
2
Q
What is activation energy? (1)
A
- The minimum energy required
for a reaction to occur (1)
3
Q
What is the maxwell Boltzmann distribution? (3)
A
- Shows the energy of gas
particles (1) - Kinetic energy on the x-axis (1)
- Number of molecules on the y-
axis (1)
4
Q
What does the area under the curve show? (1)
A
- Total number of molecules (1)
5
Q
What does the peak on the maxwell-Boltzmann curve indicate? (1)
A
- The most likely energy of a particle in a sample (1)
6
Q
What happens to the curve when temperature increases? (2)
A
- Curve shifts to the right and
has a lower peak (1) - Area under the curve stays the
same but is increased beyond
activation energy (1)
7
Q
How does temperature increase rate of reaction in terms of collision? (2)
A
- Particles have higher kinetic
energy (1) - More collisions results in more
particles having greater energy
than activation energy (1)
8
Q
How does increased pressure and concentration increase rate of reaction? (2)
A
- Particles are closer together (1)
- More frequent collisions (1)
9
Q
How do catalysts increase rate of reaction? (2)
A
- Lowers the activation energy
(1) - By providing an alternate
reaction pathway (1)
10
Q
Why are catalysts used in the industry (2)
A
- Reduces the temperature required for a reaction (1)
- Saves energy and money (1)
11
Q
What happens on the surface of heterogenous catalysts in a reaction? (3)
A
- Reactants adsorb on catalyst
surface (1) - Reaction takes place (1)
- Product desorbs from catalyst
(1)
12
Q
What happens to the activation line on the distribution curve when a catalyst is added? (1)
A
- Line shifts to the left (1)
13
Q
A
