The rate of a reaction is the change in concentration of a reactant or product divided by the time taken for the change to occur.
The rate of a reaction changes during the reaction as the reactants are used up.
Reactions are followed by measuring the change, with time, of a property that is proportional to the concentration of a reactant or product - e.g. pH of the reaction mixture, colour intensity if the reaction involves a coloured compound, volume of a gas given off.
A plot of this property against time is the progress curve for the reaction.
The half-life of a reaction is the time taken for the concentration of a reactant to decrease to one half of its initial value.
If the rate at which the reactant is used up in a reaction displays a constant half life, the reaction is first order with respect to that reactant.
The rate equation for a reaction shows how the rate of reaction varies with the concentration of each of the reactants.
Many reactions occur in a series of simple individual steps. If one step in a reaction mechanism is much slower than the others it is called the rate determining step.
Rate equations can only be predicted from the chemical equations for the individual steps in a reaction mechanism. They cannot be predicted from the overall equation for the reaction and must always be found experimentally.
1 of 3
The effect of concentration on rate (pt. 2)
For the reaction of A with B, the rate equation is given by rate=k[A]"[B]", where k is the rate constant and "(m and n) are the orders of the reation with respect to A and B. The overall order of the reaction is m+n.
In the rate experiments it is important to make measurements at a constant temperature and to investigate only one variable at a time. Other concentrations must be kept constant
To find the order of reaction with respect to a reactant A, the rate of reaction is found at different concentrations of A.
This may be done in various ways: by drawing tangents at various points on the progress curve for the reacion (the gradient of the tangent is proportional to the rate of reaction for that value of [A]), by finding the initial rate of reaction for different reaction mixtures e.g. by drawing tangents to the progress curve for each reaction mixture at the point t=0, or by using a clock technique to find the reaction time for a small amount of reaction to take place.
A graph of the rate of reaction (or quantity that is proportional to the rate of reaction) is then plotted against [A]. If the plot is a straight line, which shows that the rate is proportional to [A], the reaction is first order with respect to A.
A horizontal straight line shows that the rate is independent of [A] and so the reaction is zero order with respect to A.
2 of 3
The effect of concentration on rate (pt. 3)
Other orders give curved graphs. If the reaction is second order with respect to A, a plot of the rate against [A]squared is a straight line.
An alternative method of showing that a reaction is first order is to calculate the values of several half-lives for the reaction from the progress curve. If the values of the half-lives are euqal then the reaction is first order.
This method can only be used to check that a rection isfirst order.
The rate constant for a reaction at a particular temperature can be found by substituting values for the rate of reaction and values of [A] and [B] into the rate euqation - make sure that you used the correct units.
If you have been following the reaction by measuring a property such as pH, the rate of reaction in terms of this property must be converted to the rate of reaction in terms of concentration.
Comments
No comments have yet been made