AQA A Level Chemistry复习笔记5.2.8 Rate Determining Step

Rate-determining step & intermediates

• A chemical reaction can only go as fast as the slowest part of the reaction
  • So, the rate-determining step is the slowest step in the reaction

   

• If a reactant appears in the rate-determining step, then the concentration of that reactant will also appear in the rate equation
• For example, the rate equation for the reaction below is rate = k [CH3Br] [OH-]

CH3Br + OH- → CH3OH + Br-

• • This suggests that both CH3Br and OH- take part in the slow rate-determining step

   

• This reaction is a bimolecular reaction
  • Unimolecular: one species involved in the rate-determining step
  • Bimolecular: two species involved in the rate-determining step

   

• The intermediate is derived from substances that react together to form it in the rate-determining step
  • For example, for the reaction above the intermediate would consist of CH3Br and OH-

   

The intermediate is formed from the species that are involved in the rate-determining step (and thus appear in the rate equation)

Predicting the reaction mechanism

• The overall reaction equation and rate equation can be used to predict a possible reaction mechanism of a reaction
  • This shows the individual reaction steps which are taking place

   

• For example, nitrogen dioxide (NO2) and carbon monoxide (CO) react to form nitrogen monoxide (NO) and carbon dioxide (CO2)
  • The overall reaction equation is:

   

NO2 (g) + CO (g) → NO (g) + CO2 (g)

• • The rate equation is:

Rate = k [NO2]2

• From the rate equation it can be concluded that the reaction is zero order with respect to CO (g) and second order with respect to NO2 (g)
• This means that there are two molecules of NO2 (g) involved in the rate-determining step and zero molecules of CO (g)
• A possible reaction mechanism could therefore be:

Step 1:

2NO2 (g) → NO (g) + NO3 (g)                   slow (rate-determining step)

Step 2:

NO3 (g) + CO (g) → NO2 (g) + CO2 (g)     fast

Overall:

2NO2 (g) + NO3 (g) + CO (g) → NO (g) + NO3 (g) + NO2 (g) + CO2 (g)

=     NO2 (g) + CO (g) → NO (g) + CO2 (g)

Predicting the reaction order & deducing the rate equation

• The order of a reactant and thus the rate equation can be deduced from a reaction mechanism if the rate-determining step is known
• For example, the reaction of nitrogen oxide (NO) with hydrogen (H2) to form nitrogen (N2) and water

2NO (g) + 2H2 (g) → N2 (g) + 2H2O (l)

• The reaction mechanism for this reaction is:

Step 1:

NO (g) + NO (g) → N2O2 (g)                      fast

Step 2:

N2O2 (g) + H2 (g) → H2O (l) + N2O (g)     slow (rate-determining step)

Step 3:

N2O (g) + H2 (g) → N2 (g) + H2O (l)           fast

• The second step in this reaction mechanism is the rate-determining step
• The rate-determining step consists of:
  • N2O2 which is formed from the reaction of two NO molecules
  • One H2 molecule

   

• The reaction is, therefore, second order with respect to NO and first order with respect to H2
• So, the rate equation becomes:

Rate = k [NO]2 [H2]

• The reaction is, therefore, third order overall

Identifying the rate-determining step

• The rate-determining step can be identified from a rate equation given that the reaction mechanism is known
• For example, propane (CH3CH2CH3) undergoes bromination under alkaline solutions
• The overall reaction is:

CH3CH2CH3 + Br2 + OH- → CH3CH2CH2Br + H2O + Br-

• The reaction mechanism is:

Reaction mechanism for the bromination of propane under alkaline conditions

• The rate equation is:

Rate = k [CH3CH2CH3] [OH-]

• From the rate equation, it can be deduced that only CH3CH2CH3 and OH- are involved in the rate-determining step and not bromine (Br2)
• CH3CH2CH3 and OH- are only involved in the first step of the reaction mechanism, therefore the rate-determining step is:
  • CH3CH2CH3 + OH- → CH3CH2CH2- + H2O

   

Identifying intermediates & catalyst

• When a rate equation includes a species that is not part of the chemical reaction equation then this species is a catalyst
• For example, the halogenation of butanone under acidic conditions
• The reaction mechanism is:

• The reaction mechanism is:

Reaction mechanism of the halogenation of butanone under acidic conditions

• The rate equation is:

Rate = k [CH3CH2COCH3] [H+]

• The H+ is not a reactant in the chemical reaction equation but does appear in the rate equation
  • H+ must, therefore, be a catalyst

   

• Furthermore, the rate equation suggest that CH3CH2COCH3 and H+ must be involved in the rate-determining (slowest) step
• The CH3CH2COCH3 and H+ appear in the rate-determining step in the form of an intermediate (which is a combination of the two species)

Intermediate is formed in the rate-determining step from the reaction of CH3CH2COCH3 and H+

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