How is the rate law different from law of mass action?
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Answer :
As a chemical reaction proceeds, the concentration of the reactants decreases. The rate of reaction decreases. This implies that, the rate of reaction is directly proportional to the concentration of the reactants.
This effect of the concentration of the reactants on the rate of reaction was first studied by Guldberg and Waage. They put forward the result, called the LAW OF MASS ACTION. According to this “Law of Mass Action”, for a given reaction of the form:
aA + bB —→ Products,
the rate of reaction = k[A]^a[B]^b
where k is the equilibrium constant.
But experimentally, it has been found out that the rate of reaction may not necessarily depend on all the ‘a’ concentration terms of A or on all the ‘b’ concentration terms of B but only on some partial amount of the total concentration of A or B, say, x and y respectively.
i.e.,
Rate of Reaction = k[A]^x[B]^y
where, x and y may or may not be equal to a and b.
This above expression is called Rate Law.
Thus, Rate Law is the expression which expresses the Rate of Reaction in terms of the molar concentration of the reactants, with each term raised to a power which may or may not be equal to the stoichiometric coefficient of the reactant in the balanced chemical equation.
The Rate Law cannot be determined by just looking at the given chemical equation but, instead, can be determined only experimentally. However, the Law of Mass Action can be determined by just looking at the chemical equation.
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