kinetics

Question 1

What is the unit for rate?

Answer 1

= mol dm^-3 s-1

Question 2

What orders are possible?

Answer 2

0,1,2
0 means zero respect to that reactant
=

Question 3

How to find total orders?

Answer 3

= adding individual orders

Question 4

For a 1st order what is the overall equation for k?

Answer 4

For a 1st order overall reaction the unit of k is
= s
-1

Question 5

For a 2nd order what is the overall equation for k?

Answer 5

For a 2nd order overall reaction the unit of k is
mol-1dm3s
-1

Question 6

For a 3rd order overall reaction the unit of k is
mol-1dm3s
-1

Answer 6

= For a 3rd order overall reaction the unit of k is
mol-2dm6s
-1

Question 7

How do we find k?

Answer 7

= reerange the equation rate = k x (orders)

Question 8

How do we find units?

Answer 8

= rate / concentration
= so mol dm^3 s-1
= mol dm_3
=

Question 9

what does a large excess of reactants do?

Answer 9

= reactant will not have an affect on rate, and will be zero order
= concentration is constant

Question 10

What does the value of K mean?

Answer 10

= depends on overall orders of reaction, must be worked out from rate equation
= fixed at a particular temperature
= if temoerature changes so does k
= larger k is the faster the reaction

Question 11

What is the reason for the k constant to be like this?

Answer 11

= as temperature increases the kinetic energy increases so there is more collisions, but the concentrations remain constant

Question 12

How do we work out a order?

Answer 12

= this is only done experimentally cannot be calculaed

Question 13

What does the graph establushed by the rate equation equation lok like?

Answer 13

= x axis: log[Y]
= y axis: log rate
= log(rate)= logk + nlog[Y]

Question 14

How can a percentage error be caused?

Answer 14

= high concentrations with quick times