For the reaction A-B- product- it is found that the order of A is 1 and the order of B is 12- the concentration of both A and B are increased four times- the rate will increase by a factor of-

The correct option is B 8The Rate Law is #160; r = k[A][B]^1/2 The conc of both A and B are increased four times, the rate will increase by a factor = ...

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Standard XII

Chemistry

Rate of Reaction

For the react...

Question

For the reaction $A + B \to$ product, it is found that the order of $A$ is $1$ and the order of $B$ is $\frac{1}{2}$ , the concentration of both A and B are increased four times, the rate will increase by a factor of:

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Solution

The correct option is B 8
The Rate Law is

$r = k [A] {[B]}^{1 / 2}$

The conc of both A and B are increased four times, the rate will increase by a factor = $4 \times 4^{1 / 2}$ = $8 t i m e s$

Hence, the correct option is $B$

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For the reaction A+B→ product, it is found that the order of A is 1 and the order of B is 12, the concentration of both A and B are increased four times, the rate will increase by a factor of:

The correct option is B 8The Rate Law is r=k[A][B]1/2The conc of both A and B are increased four times, the rate will increase by a factor = 4×41/2 = 8 timesHence, the correct option is B

For the reaction $A + B \to$ product, it is found that the order of $A$ is $1$ and the order of $B$ is $\frac{1}{2}$ , the concentration of both A and B are increased four times, the rate will increase by a factor of:

The correct option is B 8
The Rate Law is

$r = k [A] {[B]}^{1 / 2}$

The conc of both A and B are increased four times, the rate will increase by a factor = $4 \times 4^{1 / 2}$ = $8 t i m e s$

Hence, the correct option is $B$