For the non - stoichiometric reaction- 2 A - B - C - D- the following kinetic data were obtained in three separate experiments- all at 298 K-Initial-Initial-Initial rate ofll-concentration-concentration-formation of - Cll - A - - B - - mol - L -1 s -1 i - 0-1 - M - 0-1 - M - 1-2 times 10-3 ll hlineii - 0-1 - M- 0-2 - M- 1-2 1-3 wend array The rate law for the formation of C isA- dC - dt - k - A - B -B- d C - dt - k - A -2- B -C- dC - dt - k - A - B -2D- d C-d t-k-A-

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Rate of Reaction

For the non -...

Question

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

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

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

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

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$\frac{d C}{d t} = k [A]$

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Solution

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

This problem can be solved by determining the order of reaction w.r.t each reactant and then writing rate law equation of the given equation accordingly as

$R = \frac{d C}{d t} = k [A]^{x} [B]^{y}$

where,
x = order of reaction w.r.t A
y = order of reaction w.r.t B

$1.2 \times 10^{- 3} = k (0.1)^{x} (0.1)^{y}$
$1.2 \times 10^{- 3} = k (0.1)^{x} (0.2)^{y}$ .....Doubling [B] had no impact on rate.This implies that change in [B] does not affect the rate. So, order w.r.t [B] is 0
$2.4 \times 10^{- 3} = k (0.2)^{x} (0.1)^{y}$ ...... Doubling [A] doubled the rate.This implies that change in [A] affects the rate linearly. So, order w.r.t [A] is 1

⇒ $R = k [A]^{1} [B]^{0}$ is the rate law for the given reaction.

⇒ $\frac{d C}{d t} = k [A]$

Suggest Corrections

Similar questions

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}

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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	$1.2 \times 10^{- 3}$
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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.

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

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.

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

The rate law for the formation of C is

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