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Chemistry (A-level)
Reaction kinetics (Chapter 2 2 )
Rate of reaction can be found by measuring the a decrease or an increase in a particular reactant or product over a period of time; unit: mol dm-3^ s-
Methods to find rate of reaction: Colorimetry can be used to monitor colour changes of a particular reactant, e.g. iodine with propanone (fading colour of iodine):
Changes in gas volume or gas pressure, e.g. benzenediazonium chloride and water:
Table 22.1 shows measurements taken at the same temperature:
[propene] means ‘concentration of propene’ Figure 22.5 showing the reaction graphically:
Concentration of propene increases from 0.00 to 0.27 mol dm-3^ in the first 5 minutes, hence average rate of reaction:
To calculate the rate at a particular point on the curve:
Calculate the gradient of the tangent (rate of reaction):
The value of -6.67 10 -4^ refers to the rate of change of cyclopropane concentration As time passes, concentration of cyclopropane falls; graph of [cyclopropane] against time:
Finding the rate of reaction through experiments (e.g. equation 3): Find the effect of H 2 (g) on the rate by varying the concentration of H 2 (g), while keeping the concentration of NO (g) constant Results show that the rate is proportional to the concentration of hydrogen (rate = k 1 [H 2 ]) Find the effect of NO (g) on the rate by varying the concentration of NO (g), while keeping the concentration of H 2 (g) constant Results show that the rate is proportional to the square of the concentration of NO (rate = k 2 [NO]^2 ) Combining gives: rate = k 1 [H 2 ] [NO]^2 The order of reaction with respect to a particular reactant is the power to which the concentration of that reactant is raised in the rate equation E.g. equation 3, first-order with respect to H 2 , second-order with respect to NO, third-order overall (as the sum of the powers is 1 + 2 = 3) For a reaction that is A + B → products, rate of reaction given by:
[A] and [B] are the concentrations of the reactants m and n are the orders of the reaction The values of m and n can be 0, 1, 2, 3 or rarely higher When the value of m or n is 0 we can ignore the concentration term because any number to the power of zero = 1.
Graph of reaction rate against concentration
For first- and second-order reactions, the graph is a curve – distinguished by determining successive half-lives of the reaction Half-life , t 1/2, is the time taken for the concentration of a reactant to fall to half its original value
Zero-order reaction has successive half-lives which decrease with time First-order reaction has a constant half-life, where half-life is independent to the concentration Second-order reaction has successive half-lives which increase with time Calculating k from half-life (first-order reactions):
t 1/2 is the half-life, units: s Rate-determining step : the slowest step in a reaction mechanism
Graph of concentration of reactant against time
Often involves changes in oxidation number of the ions involved in catalysis The catalytic role of Fe3+^ in the I-/S 2 O 8 2-^ reaction:
Fe3+^ (aq) catalyses this reaction involving two redox reactions:
The catalytic role of atmospheric oxides of nitrogen in the oxidation of atmospheric sulfur dioxide: One of the steps in the formation of acid rain is the oxidation of sulfur dioxide to sulfur trioxide:
Catalysed by nitrogen(IV) oxide
Heterogeneous catalysis occurs when the catalyst is in a different phase to the reaction mixture Often involves gaseous molecules reacting at the surface of a solid catalyst Can be explained using the theory of adsorption onto the catalyst’s surface Adsorb means to bond to the surface Absorb means to move right into the substance
Iron in the Haber process (Fe catalyst): Diffusion, adsorption, reaction and desorption
The catalytic removal of oxides of nitrogen from the exhaust gases of car engines: Adsorption, weakening of covalent bonds, formation of new bonds and desorption Small beads coated with platinum catalysts
Example questions:
sample is prevented or slowed down, e.g. by cooling the sample in ice; the concentration of one of the reactants or products is then determined by titration of the samples; common examples are the formation of an acid and an iodination reaction
