The unit of rate constant obeying the rate expression, $r = k [A] {[B]}^{2 / 3}$ is:

{m o l}^{- 2 / 3} {l i t r e}^{2 / 3} {t i m e}^{- 1}

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{m o l}^{2 / 3} {l i t r e}^{- 2 / 3} {t i m e}^{- 1}

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{m o l}^{- 5 / 3} {l i t r e}^{5 / 3} {t i m e}^{- 1}

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none of the above

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Solution

The correct option is D none of the above
The unit of rate constant is ${m o l}^{- 2 / 3} {l i t r e}^{2 / 3} {t i m e}^{2 / 3}$ and it does not match with any of the A, B, C options. So option D is correct

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Similar questions

Q. The unit of rate constant obeying the rate expression

r = K [A]^{1} [B]^{2 / 3}

is:

Q. Match the rate law given in column I with the dimensions of rate constant given in column II and mark the appropriate choice.

Column I	Column II
(A) $R a t e = k [N H_{3}]^{0}$	(i) $m o l L^{- 1} s^{- 1}$
(B) $R a t e = k [H_{2} O_{2}] [I^{-}]$	(ii) $L m o l^{- 1} s^{- 1}$
(C) $R a t e = k [C H_{3} C H O]^{3 / 2}$	(iii) $s^{- 1}$
(D) $R a t e = k [C_{2} H_{5} C l]$	(iv) $L^{1 / 2} m o l^{- 1 / 2} s^{- 1}$

Q. Read the following table and chose the appropriate option

Rate equation	Units of K
I) rate $=$ k[A]	a) mol lit $^{- 1}$ sec $^{- 1}$
II) rate $=$ k[A][B]	b) mol $^{- 2}$ lit $^{2}$ sec $^{- 1}$
III) rate $=$ k[A][B] $^{2}$	c) sec $^{- 1}$
IV) rate $=$ k	d) lit mol $^{- 1}$ sec $^{- 1}$

For the reaction, $2 A + B \to A_{2} B$ the rate $= k [A] [B]^{2}$ with $k = 2.0 \times 10^{- 6} m o l^{- 2} L^{- 2} s^{- 1}$ . Calculate the initial rate of reaction when $[A] = 0.1 m o l L^{- 1}, [B] = 0.2 m o l L^{- 1}$ . Calculate the rate of reaction after [A] is reduced to $0.06 m o l L^{- 1}$ .