For a reaction $r = K {[C H_{3} C O C H_{3}]}^{3 / 2}$ . The unit of rate of reaction and rate constant respectively is:

m o l L^{- 1} s^{- 1}, m o l^{- \frac{1}{2}} L^{\frac{1}{2}} s^{- 1}

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m o l^{- 1} L^{- 1} s^{- 1}, m o l^{- \frac{1}{2}} L^{- \frac{1}{2}} s^{- 1}

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m o l L^{- 1} s^{- 1}, m o l^{\frac{1}{2}} L^{\frac{1}{2}} s^{- 1}

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m o l L s, m o l^{\frac{1}{2}} L^{\frac{1}{2}} s

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Solution

The correct option is B $m o l L^{- 1} s^{- 1}, m o l^{- \frac{1}{2}} L^{\frac{1}{2}} s^{- 1}$
For $1.5$ order rate law the units are $m o l L^{- 1} s^{- 1}$ for the rate while the [rate constant] $= \frac{m o l L^{- 1} s^{- 1}}{m o l^{3 / 2} L^{- 3 / 2}}$
$= m o l^{- 1 / 2} L^{1 / 2} s^{- 1}$

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Similar questions

2 A + B \to A_{2} B

= k [A] [B]^{2}

k = 2.0 \times 10^{- 6} m o l^{- 2} L^{2} s^{- 1}

[A] = 0.1 m o l L^{- 1} a n d [B] = 0.2 m o l L^{- 1} i s 8 \times 10^{- 9} m o l L^{- 1} s^{- 1}

m o l L^{- 1} s^{- 1}

k = 7.06 \times 10^{- 3} {mol}^{- 1} {L s}^{- 1}

k = 5.60 \times 10^{- 5} s^{- 1}

k = 1.25 \times 10^{- 2} {mol L}^{- 1} s^{- 1}

k = 1.25 \times 10^{- 2} {mol}^{- 2} L^{2} s^{- 1}

t_{1 / 2} v / s [R]_{0}

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