RATE OF REACTION/KINETICS Flashcards
Define activation energy
Minimum energy needed for a reaction to start
What must happen for a reaction to occur
Particles must collide with E>/ Ea
Why do most collisions not cause a reaction?
Small number of particles have E>/ Ea
What is rate of reaction
Rate of chNge in concentration per unit of time
Why does increasing temperature causes incrase in rate
More particles have E>/Ea
Incrases frequency of successful collision
Why does increasing concentartion causes incrase in rate
Incrases number of particles per unit volume
Increases freqency if succlessful collissions
Why does increasing pressure causes incrase in rate
Incrases number of particles per unit volume
Increases freqency if succlessful collissions
Why does adding a catalyst increase rate
Lowers Ea
So more particles with E>/Ea
Incrases frequency of successful collision
Why does increaseing surface area causes increase in rate
Increased number of reactant particles made availabe
Increase freqency of successful collisions
Why doess small increase in temperature effect the rate of reaction
Small increase in temperature leads to significantly large number of particles with the activation energy
If the number of particles increases , how would the graph change?
The Emp & Ea would stay same
Total area under the graph would increase
What is a catalyst
Substance that increases arte if reaction but is not used up
How does a catalyst work
Providing an alternative reaction pathway that has a lower activation energy
What does 0 order mean
Chage in concentration has no effect so 0 order with respect to rate of reaction
What does 1st order mean
Concentration of reactant is directly proportional to rate
