18.1 Orders, Rate Equations, & Rate Constants

Question 1

How do you calculate the rate of a reaction?

Answer 1

change in concentration/change in time

Question 2

What are the units of rate?

Answer 2

moldm^-3s^-1

Question 3

Draw the concentration-time graph for a 0 order reaction:

Answer 3

Question 4

Draw the concentration-time graph for a first order reaction:

Answer 4

Question 5

Draw the concentration-time graph for a second order reaction:

Answer 5

Question 6

Draw the rate-concentration graph for a zero order reaction:

Answer 6

Question 7

Draw the rate-concentration graph for a first order reaction:

Answer 7

Question 8

Draw the rate-concentration graph for a second order reaction:

Answer 8

Question 9

How do you differentiate between a first and second order concentration-time graph?

Answer 9

first order has constant half-life

second order has increasing half-life

Question 10

How do you find out the initial rate from a concentration-time graph?

Answer 10

initial rate is at 0 seconds

so draw a tangent at 0 seconds, then find gradient

(change in y/change in x = concentration/time)

Question 11

How do you derive the order of a reaction?

Answer 11

carry out experiments,

each with a different concentration of reactant

to find out how the initial rate changes

Question 12

What is the overall order of a reaction?

Answer 12

sum of individual orders of each reactant

Question 13

What is the overall order of this equation?

Rate = k[A]²[B]¹[C]⁰

Answer 13

3

Question 14

What are the units of k in this reaction?

Rate = k[A]²[B]¹

Answer 14

s^-1mol^-2dm⁶

Question 15

What are the units of k in this reaction?

Rate = k[A]²[B]¹[C]¹

Answer 15

s^-1mol^-3dm⁹

Question 16

What are the units of k in this reaction?

Rate = k[A]²[B]¹[C]²

Answer 16

s^-1mol^-4dm¹²

Question 17

What are the units of k in this reaction?

Rate = k[A]

Answer 17

s^-1