Following data are obtained for the reaction- A-B- product -A-mole L-1 -B-mole L-1 Ratemole L-1 s-1 4-10-2 4-10-2 2-10-2 4-10-2 8-10-2 4-10-2 2-10-2 8-10-2 2-10-2The reaction confirms the rate law-

The correct option is C d[B]/d t = k[A] [B] ...

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Standard XII

Chemistry

Ion Electron Method

Following dat...

Question

Following data are obtained for the reaction: $A + B \to p r o d u c t$

$[A] (m o l e L^{- 1}) [B] (m o l e L^{- 1}) R a t e (m o l e L^{- 1} s^{- 1})$

$4 \times 10^{- 2} 4 \times 10^{- 2} 2 \times 10^{- 2}$
$4 \times 10^{- 2} 8 \times 10^{- 2} 4 \times 10^{- 2}$
$2 \times 10^{- 2} 8 \times 10^{- 2} 2 \times 10^{- 2}$

The reaction confirms the rate law:

- \frac{d [B]}{d t} = k [A]

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- \frac{d [B]}{d t} = k [A] {[B]}^{2}

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- \frac{d [B]}{d t} = k [A] [B]

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- \frac{d [A]}{d t} = k [B]

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Solution

The correct option is C $- \frac{d [B]}{d t} = k [A] [B]$

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Similar questions

Select the rate law that conforms to the following data for the reaction : $A + B \to P r o d u c t s$
$\begin{matrix} E x p N o . & [A] (m o l L^{- 1}) & [B] (m o l L^{- 1}) & I n i t i a l r a t e (m o l L^{- 1} S^{- 1}) 1 & 0.0012 & 0.0035 & 1 \times 10^{- 4} 2 & 0.024 & 0.070 & 8 \times 10^{- 3} 3 & 0.024 & 0.035 & 1 \times 10^{- 3} 4 & 0.012 & 0.070 & 8 \times 10^{- 3} \end{matrix}$

Q. For the non-stoichiometric reaction 2A + B ⟶ C + D. The following kinetic data were obtained in three separate experiments, all at 298 K.

Initial concentration (A)	Initial concentration (B)	Initial rate of formation of C $(m o l L^{1} S^{- 1})$
0.1M	0.1M	$1.2 \times 10^{- 3}$
0.1M	0.2M	$1.2 \times 10^{- 3}$
0.2M	0.1M	$2.4 \times 10^{- 3}$

The rate law for the formation of C is :
(IIT-JEE-2014)

Q. The rate of disappearance of

A

at two temperature is given by:

A ⇌ B

- \frac{d [A]}{d t} = 2 \times 10^{- 2} [A] - 4 \times 10^{- 3} [B]

300 K

II.

- \frac{d [A]}{d t} = 4 \times 10^{- 2} [A] - 16 \times 10^{- 4} [B]

400 K

The heat of reaction for the change is :

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Following data are obtained for the reaction: A+B→product[A](moleL−1)[B](moleL−1)Rate(moleL−1s−1)4×10−24×10−22×10−24×10−28×10−24×10−22×10−28×10−22×10−2The reaction confirms the rate law:

The correct option is C −d[B]dt=k[A][B]

The correct option is C $- \frac{d [B]}{d t} = k [A] [B]$