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The rate equation for the reaction $2 A + B \to C$ is found to be : rate = K[A][B]. The correct statement in relation to this reaction is

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$t_{\frac{1}{2}}$ is a constant

rate of formation of C is twice the rate of disappearance of A

unit of k must be $\sec^{- 1}$

value of k is independent of the initial concentrations of A and B

answer is B.

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Detailed Solution

(1) Rate = K[A][B]

Units{\text{ of K = }}\frac{{Rate}}{{\left[ A \right]\left[ B \right]}} = \frac{{mole{\text{ li}}{{\text{t}}^{ - 1}}{s^{ - 1}}}}{\left ( {mole{\text{ li}}{{\text{t}}^{ - 1}}} \right )^2} = lit\,mol{e^{ - 1}}{s^{ - 1}}

(2) Rate constant (k) depends only on temperature and catalyst.

(3) 2A + B → C

- \frac{1}{2}\frac{{d\left[ A \right]}}{{dt}} = + \frac{{d\left[ C \right]}}{{dt}}

Rate formation of 'C' is half the rate of disappearance of 'A'

(4)

for 2nd order

only option (2) is correct.

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