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Factors Affecting the Rate of a Chemical Reaction

Reaction; A...

Question

Reaction; $A + B \to C + D$ , follows rate law; $r a t e = k [A]^{\frac{1}{2}} [B]^{\frac{1}{2}}$ . Starting with initial conc, of $1 M$ of $A$ and $B$ , what is the time taken for concentration of $A$ of becomes $0.25 M$ ?
Given: $k = 2.303 \times 10^{- 3} {sec}^{- 1}$ .

A

300 s e c .

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B

600 s e c .

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C

900 s e c .

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D

1200 s e c .

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Solution

The correct option is B $600 s e c .$

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A + B ⟶ C + D

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