For a reaction of type A + B → products, it is observed that doubling concentration of Acauses the reaction rate to be four times, but doubling amount of B does not affect the rate.What will be the rate equation?
Question
For a reaction of type A + B → products, it is observed that doubling concentration of Acauses the reaction rate to be four times, but doubling amount of B does not affect the rate.What will be the rate equation?
Solution
The rate equation for a reaction is given by the formula:
Rate = k[A]^x[B]^y
where:
- Rate is the rate of reaction,
- k is the rate constant,
- [A] and [B] are the concentrations of the reactants A and B, respectively,
- x and y are the orders of the reaction with respect to A and B, respectively.
From the problem, we know that when we double the concentration of A (i.e., when we change [A] to 2[A]), the rate becomes four times. This means that the rate is proportional to the square of the concentration of A. Therefore, x = 2.
We also know that changing the concentration of B does not affect the rate. This means that the rate is not dependent on the concentration of B. Therefore, y = 0.
Substituting x = 2 and y = 0 into the rate equation, we get:
Rate = k[A]^2[B]^0
Since any number to the power of 0 is 1, [B]^0 = 1. Therefore, the rate equation simplifies to:
Rate = k[A]^2
So, the rate equation for this reaction is Rate = k[A]^2.
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