For the reaction, 2 A + B → products, when the concentration of A and B both were doubled, the rate of the reaction increased from 0.3 m o l L - 1 s - 1 to 2.4 m o l L - 1 s - 1 . When the concentration of A alone is doubled, the rate increased from 0.3 m o l L - 1 s - 1 to 0.6 m o l L - 1 s - 1 . Which one of the following statements is correct?

Order of the reaction with respect to B is 2

Total order of the reaction is 4

Order of the reaction with respect to A is 2

Order of the reaction with respect to B is 1

Under what condition the order of the reaction, 2 H I → H 2 g + I 2 g , is zero

At high partial pressure of H I

At high partial pressure of H 2

At high partial pressure of I 2

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The reaction, $L \to M$ is started with 10 g of L. After 30 and 90 minute, 5g and 1.25g of L are left respectively. The order of reaction is :

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Important Questions on Chemical Kinetics

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

For the reaction,

2 A + B \to

products, when the concentration of

A

and

B

both were doubled, the rate of the reaction increased from

0.3 m o l L^{- 1} s^{- 1}

2.4 m o l L^{- 1} s^{- 1} .

When the concentration of

A

alone is doubled, the rate increased from

0.3 m o l L^{- 1} s^{- 1}

0.6 m o l L^{- 1} s^{- 1} .

Which one of the following statements is correct?

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

The kinetic study of a reaction like $A \to P$ at $300 K$ provides the following curve, where concentration is taken in mol ${dm}^{- 3}$ and time in min.

Question Image

Identify the correct order $(n)$ and rate constant $(k)$

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

The rate constant value for a reaction is

1.75 \times 10^{2} L^{2} {mol}^{- 2} \sec^{- 1} .

The half-life period

t_{1 / 2} \propto

_______.

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

For a reaction

A + 2 B \to

Products, when concentration of

B

alone is increased, half life remains the same. If concentration of

A

alone is doubled, rate remains the same. The unit of rate constant for the reaction is

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i) and (ii)$ . The respective orders of the reaction are
(i) Question Image

(ii) Question Image

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

For the following graphs,

Question Image

Choose from the options given below, the correct one regarding order of reaction is :

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$2 NO (g) + {Cl}_{2} (g) ⇌ 2 NOCl (s)$
This reaction was studied at $- 10 ° C$ and the following data was obtained

$\begin{matrix} run & [NO]_{0} & {[{Cl}_{2}]}_{0} & r_{0} \\ 1 & 0.10 & 0.10 & 0.18 \\ 2 & 0.10 & 0.20 & 0.35 \\ 3 & 0.20 & 0.20 & 1.40 \end{matrix}$

$[NO]_{0}$ and ${[{Cl}_{2}]}_{0}$ are the initial concentrations and $r_{0}$ is the initial reaction rate. The overall order of the reaction is
(Round off to the Nearest Integer).

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

For the reaction,

X + Y \to

Products, the following data is obtained at

300 K

Experiment Number	Initial concentration in $(mol L^{- 1})$		Rate (in $mol L^{- 1} \min^{- 1}$ )
Experiment Number	$[X]$	$[Y]$	Rate (in $mol L^{- 1} \min^{- 1}$ )
$1$	$0.010$	$0.010$	$1.2 \times 10^{- 4}$
$2$	$0.010$	$0.020$	$2.4 \times 10^{- 4}$
$3$	$0.020$	$0.020$	$9.6 \times 10^{- 4}$

The order of the reaction is

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

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 reactions is:

$[A] (m o l L^{- 1})$	$[B] (m o l L^{- 1})$	$I n i t i a l R a t e$ $(m o l L^{- 1} s^{- 1})$
0.05	0.05	0.045
0.10	0.05	0.090
0.20	0.10	0.72

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

The rate law for the reaction

2 {NO}_{(g)} + O_{2 (g)} ⟶ 2 {NO}_{2 (g)}

is rate

= k [NO]^{2} [O_{2}]

, then which among the following statement is correct?

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The following data was obtained for chemical reaction given below at $975 K$ .

$2 {NO}_{(g)} + 2 H_{2 (g)} \to N_{2 (g)} + 2 H_{2} O_{(g)}$

$\begin{matrix} [NO] & [H_{2}] & Rate \\ mol L^{- 1} & mol L^{- 1} & {molL}^{- 1} s^{- 1} \\ (A) & 8 \times 10^{- 5} & 8 \times 10^{- 5} & 7 \times 10^{- 9} \\ (B) & 24 \times 10^{- 5} & 8 \times 10^{- 5} & 2.1 \times 10^{- 8} \\ (C) & 24 \times 10^{- 5} & 32 \times 10^{- 5} & 8.4 \times 10^{- 8} \end{matrix}$

The order of the reaction with respect to $NO$ _____ is [Integer answer]

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

The data given below are for the reaction of

A

and

D_{2}

to form product at

295 K

. Find the correct rate expression for this reaction

$\frac{D_{2}}{m o l L^{- 1}}$	$\frac{A}{m o l L^{- 1}}$	$\frac{I n i t i a l r a t e}{m o l L^{- 1} s^{- 1}}$
$0.05$	$0.05$	$1 \times 10^{- 3}$
$0.15$	$0.05$	$3 \times 10^{- 3}$
$0.05$	$0.15$	$9 \times 10^{- 3}$

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

For the reaction $2 A + B_{2} ⟶ 2 C,$ the following data is provided. Find the overall order of this reaction.

Experiment	$[A] (mol \cdot L^{- 1})$	$[B] (mol . L^{- 1})$	$(mol . L^{- 1} \cdot s^{- 1})$
$1$	$0.5$	$0.5$	$1 \times 10^{- 4}$
$2$	$0.5$	$1.0$	$2 \times 10^{- 4}$
$3$	$1.0$	$1.0$	$2 \times 10^{- 4}$

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

If 50 % of a reaction occurs in 100 second and 75 % of the reaction occurs in 200 second, the order of this reaction is:

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

What will be the overall order of a reaction for which the rate expression is given as
Rate

= K [A]^{\frac{1}{2}} [B]^{\frac{3}{2}}

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What is the order with respect to [A], [B] and [C], respectively?

[A]	[B]	[C]	Rate $[M / \sec]$
$0.2$	$0.1$	$0.02$	$8.08 \times 10^{- 3}$
$0.1$	$0.2$	$0.02$	$2.01 \times 10^{- 3}$
$0.1$	$1.8$	$0.18$	$6.03 \times 10^{- 3}$
$0.2$	$0.1$	$0.08$	$6.464 \times 10^{- 2}$

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

345 K

, the half life for the decomposition of a sample of a gaseous compound initially at

55.5 kPa

was

340 s

. When the pressure was

27.8 kPa

, the half life was found to be

170 s

. The order of the reaction is - [integer answer]

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

For a reaction

2 A + B \to P,

when concentration of

B

alone is doubled,

t_{1 / 2}

does not change and when concentrations of both

A

and

B

is doubled, rate increases by a factor of

4 .

The unit of rate constant is,

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Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

518^{o} C,

the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of

363 Torr

was

1 .00 Torr s^{- 1}

when

5 %

had reacted and

0 .50 Torr s^{- 1}

when 33% had reacted. The order of the reaction is:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Determination of Order of Reaction

Under what condition the order of the reaction,

2 H I \to H_{2} (g) + I_{2} (g),

is zero

The reaction, L → M is started with 10 g of L. After 30 and 90 minute, 5g and 1.25g of L are left respectively. The order of reaction is :

Important Questions on Chemical Kinetics

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The reaction, $L \to M$ is started with 10 g of L. After 30 and 90 minute, 5g and 1.25g of L are left respectively. The order of reaction is :