Select the rate law that corresponds to the data shown for the following reaction- A-B- CExpt-No -A-0 -B-0Initial rate1-0-0120-0350-102-0-0240-0700-803-0-0240-0350-104-0-0120-0700-80

The correct option is A rate= k[B]^3 Reaction : #160; A+B→ C When [A] is doubled or not changed, rate of reaction is not affected but when [B] is dou ...

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Standard XII

Chemistry

Zero Order Reaction

Select the ra...

Question

Select the rate law that corresponds to the data shown for the following reaction: $A + B \to C$
Expt.No $[A]_{0}$ $[B]_{0}$ Initial rate
1. 0.012 0.035 0.10
2. 0.024 0.070 0.80
3. 0.024 0.035 0.10
4. 0.012 0.070 0.80

rate=

k [B]^{3}

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rate=

k [B]^{4}

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rate=

k [A] [B]^{3}

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rate=

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

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Solution

The correct option is A rate= $k [B]^{3}$
Reaction : $A + B \to C$

When [A] is doubled or not changed, rate of reaction is not affected but when [B] is doubled, rate of reaction increases by power of 3.

So, the rate law becomes : $r a t e = k [A]^{0} [B]^{3}$ .

Hene, Option "A" is the correct answer.

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Similar questions

Q. For the reaction

2 A + B \to C

, the values of initial rate at different reactant concentrations are given in the table below: The rate law for the reaction is:

$[A] (m o l L^{- 1})$	$[B] (m o l L^{- 1})$	$Initial Rate (m o l L^{- 1} s^{- 1})$
0.05	0.05	0.045
0.10	0.05	0.090
0.20	0.10	0.72

Q. Select the rate law that corresponds to the data shown for the following reaction:

A + B \to C

Exp.	$[A]$	$[B]$	Initial rate
$1$ .	$0.012$	$0.035$	$0.10$
$2$ .	$0.024$	$0.070$	$1.6$
$3$ .	$0.024$	$0.035$	$0.20$
$4$ .	$0.012$	$0.070$	$0.80$

Q. For the reaction A + B

\to

C; starting with different initial concentration of A and B, initial rate of reaction were determined graphically in four experiments.

\begin{matrix} S l . N o & [A]_{0} / M (I n i t i a l c o n c .) & [B]_{0} / M (I n i t i a l c o n c .) & R a t e / (M s e c^{- 1}) 1. & 1.6 \times 10^{- 3} & 5 \times 10^{- 2} & 10^{- 3} 2. & 3.2 \times 10^{- 3} & 5 \times 10^{- 2} & 4 \times 10^{- 3} 3. & 1.6 \times 10^{- 3} & 10^{- 1} & 2 \times 10^{- 3} 4. & 3.2 \times 10^{- 3} & 10^{- 1} & 8 \times 10^{- 3} \end{matrix}

Rate law for reaction from above data is

Q. Select the rate law that corresponds to the data shown for the following reaction:

A + B ⟶ C

Exp	$[A]$	$[B]$	$I n i t i a l R a t e$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

Q. For a reaction

A + 2 B \to C + D

, the following data were obtained

The correct rate law expression will be

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Expt.No	$[A]_{0}$	$[B]_{0}$	Initial rate
1.	0.012	0.035	0.10
2.	0.024	0.070	0.80
3.	0.024	0.035	0.10
4.	0.012	0.070	0.80

Select the rate law that corresponds to the data shown for the following reaction: A+B→CExpt.No[A]0[B]0Initial rate1.0.0120.0350.102.0.0240.0700.803.0.0240.0350.104.0.0120.0700.80

The correct option is A rate=k[B]3Reaction : A+B→CWhen [A] is doubled or not changed, rate of reaction is not affected but when [B] is doubled, rate of reaction increases by power of 3.So, the rate law becomes : rate=k[A]0[B]3.Hene, Option "A" is the correct answer.

Select the rate law that corresponds to the data shown for the following reaction: $A + B \to C$
Expt.No $[A]_{0}$ $[B]_{0}$ Initial rate
1. 0.012 0.035 0.10
2. 0.024 0.070 0.80
3. 0.024 0.035 0.10
4. 0.012 0.070 0.80