For a reaction A -2 B - C - D- the following data were obtained 3-c- Experimental Initial Concentration m o l L -1 Initial rate of formation of D m o l L -1 m i n - 1 A B 1- 0-1 0-1 6-0 - 10-3 2 - 0-3 0-2 7-2 - 10-2 3- 0-3 0-4 2-88 - 10-1 4 - 0-4 0-1 2-4 - 10-2 The correct rate law expression will beA- Rate - k - A - B -2B- Rate - k - A -2- B -2C- Rate - k - A - B -D- Rate - k - A -2- B -

The correct option is A Rate = k [A] [B]^2r = k[A]^x [B]^y 6.0 × 10^ 3 = K(0.1)^x (0.1)^y (1) 2.4 × 10^ 2 =K (0.4)^x (0.1)^y (2) (2)/(1) gives ...

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Standard XII

Chemistry

Factors Affecting Rate of Reaction

For a reactio...

Question

For a reaction $A + 2 B \to C + D$ , the following data were obtained

The correct rate law expression will be

Rate = k [A] [B]

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

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

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

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Solution

The correct option is B $Rate = k [A] [B]^{2}$
$r = k [A]^{x} [B]^{y}$

$6.0 \times 10^{- 3} = K (0.1)^{x} (0.1)^{y} - (1)$

$2.4 \times 10^{- 2} = K (0.4)^{x} (0.1)^{y} - (2)$

$\frac{(2)}{(1)}$ gives $x = 1$

$7.2 \times 10^{- 2} = K (0.3)^{x} (0.2)^{y} - (3)$

$2.88 \times 10^{- 1} = K (0.3)^{x} (0.4)^{y} - (4)$

$\frac{(4)}{(3)}$ gives $y = 2$

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Similar questions

The following results have been obtained during the kinetic studies of the reaction:

2A + B → C + D

Experiment	A/ mol L⁻¹	B/ mol L⁻¹	Initial rate of formation of D/mol L⁻¹ min⁻¹
I	0.1	0.1	6.0 × 10⁻³
II	0.3	0.2	7.2 × 10⁻²
III	0.3	0.4	2.88 × 10⁻¹
IV	0.4	0.1	2.40 × 10⁻²

Determine the rate law and the rate constant for the reaction.

Q. For a reaction

A + 2 B \to C + D

, the following data were obtained.
Excpt. Initial concentration Initial Rate of formation of D
(moles

{l i t r e}^{- 1}

)

{l i t r e}^{- 1} {m i n}^{- 1}

)
[A] [B]
1.

0.1

0.1

6.0 \times 10^{- 3}

0.3

0.2

7.2 \times 10^{- 2}

0.3

0.4

2.8 \times 10^{- 1}

0.4

0.1

2.4 \times 10^{- 2}

The correct rate law expression will be:

Q. The following results have been obtained during the kinetic study of the reaction

A + B ⟶ C + D

\begin{matrix} Experiment & [A] & [B] & Initial rate of formation of (M s e c^{- 1}) I & 0.1 & 0.1 & 6.0 \times 10^{- 3} II & 0.3 & 0.2 & 7.2 \times 10^{- 2} III & 0.3 & 0.4 & 2.88 \times 10^{- 1} IV & 0.4 & 0.1 & 2.40 \times 10^{- 2} \end{matrix}

Determine the rate law of the above reaction.

Q. The following results have been obtained during the kinetic studies of the reaction:

2 A + B \to C + D

Experiment	$[A] / m o l L^{- 1}$	$[B] / m o l L^{- 1}$	Initial rate of formation of $D / m o l L^{- 1} m i n^{- 1}$
I	$0.1$	$0.1$	$6.0 \times 10^{- 3}$
II	$0.3$	$0.2$	$7.2 \times 10^{- 2}$
III	$0.3$	$0.4$	$2.88 \times 10^{- 1}$
IV	$0.4$	$0.1$	$2.40 \times 10^{- 2}$

Determine the rate law and the rate constant for the reaction.

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 a reaction A+2B→C+D, the following data were obtained The correct rate law expression will be

The correct option is B Rate=k[A][B]2r=k[A]x[B]y 6.0×10−3=K(0.1)x(0.1)y − (1) 2.4×10−2=K(0.4)x(0.1)y − (2) (2)(1) gives x=1 7.2×10−2=K(0.3)x(0.2)y − (3) 2.88×10−1=K(0.3)x(0.4)y − (4) (4)(3) gives y=2

For a reaction $A + 2 B \to C + D$ , the following data were obtained

The correct rate law expression will be