Kinetics Flashcards
1
Q
Define reaction rate
A
Change in conc of R/P over time
2
Q
Rate of reaction equation
A
Rate of reaction = amount of R or product / time
3
Q
Explain what happens for a reaction to occur
A
- When collisions take place btw particles
- Must have enough activation energy
- Energy needed to break bonds
4
Q
Define activation energy
A
The minimum amount of kinetic energy that particles need to react
5
Q
State the effect of increasing the temperature on the rate of reaction
A
- Larger proportion of particles
- have enough activation energy
- freq. successful collisions inc
- ROR inc
6
Q
State the effect of increasing the conc on the rate of reaction
A
- More particles
- freq. successful collisions inc
- ROR inc
7
Q
State the effect of increasing the pressure on the rate of reaction
A
- More particles
- freq. successful collisions inc
- ROR inc
8
Q
Define catalyst
A
Substance that inc ROR by providing alternative route w/ lower activation energy. Chemically unchanged at end of reaction
9
Q
Why does lowering the activation energy inc rate of reaction?
A
- More particles will have energy > Ea
- Higher freq. sucessful collisions
10
Q
Outline the practical to investigate the effect of temperature on the rate of reaction
A
- Sodium thiosulfate + HCL (colourless sol) → sulfur (yellow ppt)
- Measure fixed vol of ST + HCL in measuring cylinder
- Use water bath + heat gently til desired temp reached
- Mix sol in clonical flask, put ontop of paper w/ x
- Time til X is no longer visible
- Repeat at diff temp
- Higher temp, faster ROR
