The reaction between A and B is first order with respect to A and zero order with respect to B. Analyse the given data for the same reaction.
Experiment
[A] inmol $L^{- 1}$
[B] inmol $L^{- 1}$ Initial rate in mole $L^{- 1} m i n^{- 1}$
I
0.1
0.1
$2 \times 10^{- 2}$
II
-
0.2
$4 \times 10^{- 2}$
III
0.4
0.4
-
IV
-
0.2
$2 \times 10^{- 2}$
Which of the folllowing is/are correct for the above data :

Concentration of A in II experiment is

1 \times 10^{- 1} m o l L^{- 1}

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Half life period of B is independent of initial concentration.

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Initial rate for experiment III is

3.2 \times 10^{- 2} m o l L^{- 1} m i n^{- 1}

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Concentration of A in experiment IV is

5 \times 10^{- 2} m o l L^{- 1}

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Solution

The correct options are
B Concentration of A in II experiment is $1 \times 10^{- 1} m o l L^{- 1}$
D Concentration of A in experiment IV is $5 \times 10^{- 2} m o l L^{- 1}$
$r a t e = k [A] [B]^{0}$
I $2 \times 10^{- 2} = k [0.1]^{1}$
II $4 \times 10^{- 2} = k [A]^{1}$
III $r a t e = k [0.4]^{1}$
IV $2 \times 10^{- 2} = k [A]^{1}$
option A and D are correct

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Similar questions

Q. The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:

Experiment	$[A] / m o l L^{- 1}$	$B] / m o l L^{- 1}$	Initial rate/ $m o l L^{- 1} m i n^{- 1}$
I	$0.1$	$0.1$	$2.0 \times 10^{- 2}$
II	-	$0.2$	$4.0 \times 10^{- 2}$
III	$0.4$	$0.4$	-
IV	-	$0.2$	$2.0 \times 10^{- 2}$

The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:

Experiment	A/ mol L⁻¹	B/ mol L⁻¹	Initial rate/mol L⁻¹ min⁻¹
I	0.1	0.1	2.0 × 10⁻²
II	--	0.2	4.0 × 10⁻²
III	0.4	0.4	--
IV	--	0.2	2.0 × 10⁻²

The reation between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:

$\begin{matrix} E x p e r i m e n t & [A] m o l L^{- 1} & [B] m o l L^{- 1} & I n i t i a l r a t e m o l L^{- 1} m i n^{- 1} I & 0.1 & 0.1 & 2.0 \times 10^{- 2} I I & - & 0.2 & 4.0 \times 10^{- 2} I I I & 0.4 & 0.4 & - I V & - & 0.2 & 2.0 \times 10^{- 2} \end{matrix}$

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.

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

2 A + B \to P r o d u c t s

Experiment	[A] (in mol $L^{- 1}$	[B] (in mol $L^{- 1}$ )	Initial rate of the reaction (in mol $L^{- 1} m i n^{- 1}$ )
(I)	0.10	0.20	6.93x $10^{- 3}$
(II)	0.10	0.25	6.93x $10^{- 3}$
(III)	0.20	0.30	1.386x $10^{- 2}$

The time (in minutes) required to consume half of A is:

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Experiment	[A] inmol $L^{- 1}$	[B] inmol $L^{- 1}$	Initial rate in mole $L^{- 1} m i n^{- 1}$
I	0.1	0.1	$2 \times 10^{- 2}$
II	-	0.2	$4 \times 10^{- 2}$
III	0.4	0.4	-
IV	-	0.2	$2 \times 10^{- 2}$

The correct options are B Concentration of A in II experiment is 1×10−1molL−1 D Concentration of A in experiment IV is 5×10−2molL−1rate=k[A][B]0I 2×10−2=k[0.1]1II 4×10−2=k[A]1III rate=k[0.4]1IV 2×10−2=k[A]1option A and D are correct