For the non-stoichiometre reaction $2 A + B \to C + D,$ the following kinetic data were obtained in three seperate experiments, all at $298 K .$ The rate law for the formation of $C$ is:

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

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\frac{d c}{d t} = k [A]

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

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

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Solution

The correct option is B $\frac{d c}{d t} = k [A]$
$R a t e, r = k [A]^{x} [B]^{y}$
$1.2 \times 10^{- 3} = k [0.1]^{x} [0.1]^{y}$ ----- 1
$1.2 \times 10^{- 3} = k [0.1]^{x} [0.2]^{y}$ ----- 2
$2.4 \times 10^{- 3} = k [0.2]^{x} [0.1]^{y}$ ----- 3
Solving equation 1 and 2 we get $y = 0$

Solving equation 1 and 3 we get $x = 1$

So, $x = 1, y = 0$
$R a t e, r = k [A]$

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Similar questions

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)

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

$\begin{matrix} I n i t i a l & I n i t i a l & I n i t i a l r a t e o f c o n c e n t r a t i o n & c o n c e n t r a t i o n & f o r m a t i o n o f C [A] & [B] & (m o l L^{- 1} s^{- 1}) (i) & 0.1 M & 0.1 M & 1.2 \times 10^{- 3} (i i) & 0.1 M & 0.2 M & 1.2 \times 1^{- 3} (i i i) & 0.2 M & 0.1 M & 2.4 \times 10^{- 3} \end{matrix}$

The rate law for the formation of C is

Q. For the non – stoichimetric reaction,

2 A + B \to C + D,

the following kinetic data were obtained in three separate experiments, all at 298 K.

\begin{matrix} I n i t i a l C o n c e n t r a t i o n & I n i t i a l C o n c e n t r a t i o n & I n i t i a l r a t e o f F o r m a t i o n o f C (A) & (B) & (m o l L^{- 1} s^{- 1}) 0.1 M & 0.1 M & 1.2 \times 10^{- 3} 0.1 M & 0.2 M & 1.2 \times 10^{- 3} 0.2 M & 0.1 M & 2.4 \times 10^{- 3} \end{matrix}

The rate law for the formation of C is

Q. For the non - stoichiometric relation :

2 A + B \to C + D

, the following kinetic data was obtained in the seperate experiments, all at 298 K.

\begin{matrix} Initial concentration & Initial concentration & Initial rate of formation [A] & [B] & {(mol L}^{- 1} s^{- 1}) 0.1 M & 0.1 M & 1.2 \times 10^{- 3} 0.1 M & 0.2 M & 1.2 \times 10^{- 3} 0.2 M & 0.1 M & 2.4 \times 10^{- 3} \end{matrix}

The rate law for the formation of

C

is:

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

$\begin{matrix} Initial & Initial & Initial rate of concentration & concentration & formation of C [A] & [B] & (m o l L^{- 1} s^{- 1}) (i) & 0.1 M & 0.1 M & 1.2 \times 10^{- 3} (i i) & 0.1 M & 0.2 M & 1.2 \times 1^{- 3} (i i i) & 0.2 M & 0.1 M & 2.4 \times 10^{- 3} \end{matrix}$ The rate law for the formation of C is

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For the non-stoichiometre reaction 2A+B→C+D, the following kinetic data were obtained in three seperate experiments, all at 298K. The rate law for the formation of C is:

The correct option is B dcdt=k[A]Rate,r=k[A]x[B]y1.2×10−3=k[0.1]x[0.1]y ----- 11.2×10−3=k[0.1]x[0.2]y ----- 22.4×10−3=k[0.2]x[0.1]y ----- 3Solving equation 1 and 2 we get y=0Solving equation 1 and 3 we get x=1So, x=1, y=0Rate,r=k[A]

For the non-stoichiometre reaction $2 A + B \to C + D,$ the following kinetic data were obtained in three seperate experiments, all at $298 K .$ The rate law for the formation of $C$ is: