Consider the following reaction, the rate expression of which is given below A + B → C rate = k [ A ] 1/2 [ B ] 1/2 The reaction is initiated by taking 1 M concentration of A and B each. If the ra

Question

Consider the following reaction, the rate expression of which is given below $A + B \to C rate = k [A]^{1/2} [B]^{1/2}$ The reaction is initiated by taking $1 M$ concentration of $A$ and $B$ each. If the rate constant $(k)$ is $4.6 \times 1 0^{- 2} s^{- 1}$ , then the time taken for $A$ to become $0.1 M$ is ______ sec. (nearest integer)

Answer:

50.00

Solution:

$K = \frac{2.303}{t} lo g \frac{1}{0.1} 4.6 \times 1 0^{- 2} = \frac{2.303}{t} t = 50 sec .$

TestHub · Accepted Answer

​ K = t 2.303 ​ lo g 0.1 1 ​ 4.6 × 1 0 − 2 = t 2.303 ​ t = 50 sec . ​

Chemistry - Chemical Kinetics Question with Solution | TestHub

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