Rate Law
We know that the rate law is the expression in which reaction rate is given in terms of molar concentration of reactants with each term raised to some power, which may or may not be equal to the stoichiometric coefficient of the reacting species in a balanced chemical equation.
Consider a general reaction, aA + bB → cC + dD where a, b, c, d are the stoichiometric coefficients of the reactants and products. Therefore, the rate law for this reaction is,
Rate ∝ [A]x [B]y
where x and y may or may not be equal to the stoichiometric coefficients of the reactants. Therefore, the rate of the reaction is equal to k [A]x [B]y, where k is the rate constant.
∴ -d[R]/dt = k [A]x [B]y
Order of Reaction
Order of a reaction is the sum of the powers of the concentrations of the reactants in the rate law expression. In the above general reaction, x and y are the powers. The sum of them will give the order of the reaction. Order of a reaction can be 0, 1, 2, 3 and even a fraction. A zero-order reaction means that the rate of the reaction is independent of the concentration of reactants.
Zero Order Reaction
So we already know that in a zero order reaction, the rate is independent of the concentration of the reactants. Thus, it means the sum of the powers of concentrations is zero. It can only be zero when the all the powers are zero. Consider a reaction, R → P. Therefore, the rate law of this reaction is,
Rate ∝ [R]0
∴ Rate = -d[R]/dt = k[R]0 = k × 1
∴ Rate = -d[R]/dt = k
∴ d[R] = -kdt
Integrating both sides, [R] = -kt + I……………….(I)
where I is the constant if integration. At t = 0, the concentration of the reactant R = [R]0.where [R]0 is the initial concentration of the reactant. Substituting this value in the equation I,
[R]0 = -k ×0 + I = I
Substituting this value of I in the equation (I), we get
[R] = -kt + [R]0 ………………(II)
Comparing equation II with the equation of a straight line y= mx +c, if we plot [R] against t, we get a straight line with slope = -k and intercept = [R]0
(Source: askiitians.com)
Therefore, on simplifying equation II, we get
k ={ [R]0 – [R]}/t……………..(III)
Example of Zero Order Reaction
Zero-order reactions are very uncommon but they occur under certain condition. An example of a zero-order reaction is decomposition of ammonia, 2NH3 → N2 + 3H2
Rate = k[NH3]0 = k
First Order Reaction
In this type of reaction, the sum of the powers of concentrations of reactants in rate law is equal to 1, that is the rate of the reaction is proportional to the first power of the concentration of the reactant. Consider the reaction R → P again. Therefore, the rate law for this reaction is,
Rate ∝ [R]
We know that [R] = -kt + [R]0 ( from equation II). Taking log of both sides, we get
ln[R] = -kt + ln[R]0 ………………………….(IV)
∴ ln[R]/[R]0 = -kt …………………………….(V)
∴ k = (1/t) ln [R]0 /[R] ………………………(VI)
Now, consider equation II again. At time t1 and time t2, the equation II will be [R]1 = -kt1 + [R]0 and [R]2 = -kt2 + [R]0 respectively, where [R]1 and [R]2 are concentrations of the reactants at time t1 and t2 respectively. Subtracting second equation from first one, we get
ln [R]1– ln[R]2 = -kt1 – (- kt2 )
∴ ln[R]1 /[R]2 = k (t2 – t1)
∴ k = [1/(t2 – t1)] ln[R]1 /[R]2
Now, taking antilog of both sides of equation V, we get [R] = [R]0e-kt
Comparing this equation with equation of a straight line y = mx + c, if we plot ln [R] against t, we get a straight line with slope = -k and intercept = ln[R]0
(Source: nonsibihighschool.org)
On removing natural logarithm from equation VI, the first-order reaction can also be written as,
k = 2.303/t log[R]0 /[R] …………..(VII)
If we plot a graph of log[R]0 /[R] against t, we get slope = k/2.303
Example of First Order Reaction
An example of a first-order reaction is hydrogenation of ethene.
C2H4 + H2 → C2H6
Therefore the rate of reaction = k [C2H4]. Hence, equations III and VII are the equations of rate constants of zero and first order reactions respectively. We can find rate constants, initial and final concentrations and the time taken for the reaction to occur using these reactions.
A Solved Question for You
Q: The order of a reaction is:
a) can never be zero b) can never be a fraction
c) must be a whole number only d) can be a whole number or a fraction or zero
Solution: d) can be a whole number or a fraction or zero. It depends on the dependency of the rate of reaction on the reactants. If the rate is independent of the reactants, then the order of reaction is zero. Therefore, the rate law of a zero order reaction would be rate α [R]0 where [R] is the concentration of the reactant.
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