18.1 Orders, Rate Equations, & Rate Constants
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How do you calculate the rate of a reaction?
change in concentration/change in time
What are the units of rate?
moldm-3s-1
Draw the concentration-time graph for a 0 order reaction:
Draw the concentration-time graph for a first order reaction:
Draw the concentration-time graph for a second order reaction:
Draw the rate-concentration graph for a zero order reaction:
Draw the rate-concentration graph for a first order reaction:
Draw the rate-concentration graph for a second order reaction:
How do you differentiate between a first and second order concentration-time graph?
first order has constant half-life second order has increasing half-life
How do you find out the initial rate from a concentration-time graph?
initial rate is at 0 seconds so draw a tangent at 0 seconds, then find gradient (change in y/change in x = concentration/time)
How do you derive the order of a reaction?
carry out experiments, each with a different concentration of reactant to find out how the initial rate changes
What is the overall order of a reaction?
sum of individual orders of each reactant
What is the overall order of this equation? Rate = k[A]2[B]1[C]0
3
What are the units of k in this reaction? Rate = k[A]2[B]1
s-1mol-2dm6
What are the units of k in this reaction? Rate = k[A]2[B]1[C]1
s-1mol-3dm9
What are the units of k in this reaction? Rate = k[A]2[B]1[C]2
s-1mol-4dm12
What are the units of k in this reaction? Rate = k[A]
s-1