Thermal decomposition of N 2 O 5 occurs as per the equation below : 2 N 2 O 5 → 4 NO 2 + O 2 The correct statement is

rate of disappearance of N 2 O 5 is twice the O 2 production rate

O 2 production rate is four times the NO 2 production rate

O 2 production rate is the same as the rate of disappearance of N 2 O 5

rate of disappearance of N 2 O 5 is one-fourth of NO 2 production rate

For the reaction 2 A + 3 B + 3 2 C → 3 P , which statement is correct?

dn A dt = 2 3 dn B dt = 4 3 dn C dt

d n A d t = 3 2 d n B d t = 3 4 d n C d t

dn A dt = 2 3 dn B dt = 3 4 dn C dt

Ammonia and oxygen react at high temperature as; 4 NH 3 g + 5 O 2 ( g ) → 4 NO ( g ) + 6 H 2 O ( g ) In an experiment rate of formation NO is 3 . 6 × 10 - 3 mol L - 1 s - 1 . Calculate rate of disappearance of ammonia.

3 . 6 × 10 - 3 mol L - 1 s - 1

The following results have been obtained during the kinetic studies of reaction: 2 NO + 2 H 2 ⟶ N 2 + 2 H 2 O Expt - d [ NO ] dt molL - 1 s - 1 [ NO ] molL - 1 H 2 molL - 1 1 . 4 . 8 × 10 - 5 1 × 10 - 2 1 × 10 - 3 2 . 43 . 2 × 10 - 5 3 × 10 - 2 1 × 10 - 3 3 . 86 . 4 × 10 - 5 3 × 10 - 2 2 × 10 - 3

- d [ NO ] dt = k [ NO ] 2 H 2 1 2

For an elementary reaction 2 A + 3 B → 4 C + D the rate of appearance of C at time ' t ' is 2 . 8 × 10 - 3 mol L - 1 S - 1 . Rate of disappearance of B at ' t ' , t will be

3 4 2 . 8 × 10 - 3 molL - 1 S - 1

2 2 . 8 × 10 - 3 molL - 1 S - 1

1 4 2 . 8 × 10 - 3 molL - 1 S - 1

4 3 2 . 8 × 10 - 3 molL - 1 S - 1

For the reaction, 3A + 2B → C + D , the differential rate law can be written as :

- 1 3 d A dt = d C dt = k A n B m

+ 1 3 d A dt = - d C dt = k A n B m

1 3 d A dt = d C dt = k A n B m

MEDIUM

Earn 100

For a reaction $\frac{d x}{d t} = K {[H^{+}]}^{n}$ . If $p H$ of the reaction medium changes from two to one the rate becomes $100 t i m e s$ of value at $p H = 2$ . What is the order of reaction?

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Important Questions on Chemical Kinetics

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

For the reaction,

2 {SO}_{2} + O_{2} ⇌ 2 {SO}_{3}

, The rate of disappearance of

O_{2}

2 \times 10^{- 4} mol L^{- 1} s^{- 1}

. The rate of appearance of

{SO}_{3}

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

In the reaction,

N_{2} + 3 H_{2} ⟶ 2 {NH}_{3}

, the rate of disappearance of

H_{2}

0.02 M / s

. The rate of appearance of

{NH}_{3}

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

Thermal decomposition of $N_{2} O_{5}$ occurs as per the equation below :

$2 N_{2} O_{5} \to 4 {NO}_{2} + O_{2}$

The correct statement is

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

For a reaction

1 / 2 A \to 2 B

, rate of disappearance of

A

is related to rate of appearance of

B

by the expression

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

For the reaction

2 A + 3 B + \frac{3}{2} C \to 3 P

, which statement is correct?

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

Ammonia and oxygen react at high temperature as;

4 {NH}_{3}_{(g)} + 5 {O_{2}}_{(g)} \to 4 {NO}_{(g)} + 6 H_{2} O_{(g)}

In an experiment rate of formation

NO

3.6 \times 10^{- 3} mol L^{- 1} s^{- 1}

. Calculate rate of disappearance of ammonia.

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

The following results have been obtained during the kinetic studies of reaction:
$2 NO + 2 H_{2} ⟶ N_{2} + 2 H_{2} O$

Expt	$\frac{- d [NO]}{dt}$ ${molL}^{- 1} s^{- 1}$	$[NO]$ ${molL}^{- 1}$	$[H_{2}]$ ${molL}^{- 1}$
$1$ .	$4.8 \times 10^{- 5}$	$1 \times 10^{- 2}$	$1 \times 10^{- 3}$
$2$ .	$43.2 \times 10^{- 5}$	$3 \times 10^{- 2}$	$1 \times 10^{- 3}$
$3$ .	$86.4 \times 10^{- 5}$	$3 \times 10^{- 2}$	$2 \times 10^{- 3}$

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

For the non-stoichiometry reaction,

2 A + B \to 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 $({mol L}^{-} S^{-})$
$0.1 M$	$0.1 M$	$1.2 \times 1 0^{- 3}$
$0.1 M$	$0.2 M$	$1.2 \times 1 0^{- 3}$
$0.2 M$	$0.1 M$	$2.4 \times 1 0^{- 3}$

The rate law for the formation of

C

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

For the reaction

N_{2} + 3 H_{2} \to 2 {NH}_{3}

, if

\frac{Δ [{NH}_{3}]}{Δt} = 2 \times 10^{- 4} mol L^{- 1} s^{- 1},

the value of

\frac{- Δ [H_{2}]}{Δt}

would be

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

Given the hypothetical reaction mechanism

$A \overset{I}{⟶} B \overset{II}{⟶} C \overset{III}{⟶} D \overset{IV}{\to} E$ and the rate as

Species formed	Rate of its information
$B$	$0.002 mol / h$ per mole of $A$
$C$	$0.030 mol / h$ per mole of $B$
$D$	$0.011 mol / h$ per mole of $C$
$E$	$0.420 mol / h$ per mole of $D$

The rate determining step is

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

Decomposition of

X

exhibits a rate constant of

0 .05 μg / year

. How many years are required for the decomposition of

5 μg

X

into

2 .5 μg

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

For a reaction scheme

A \overset{k_{1}}{\to} B \overset{k_{2}}{\to} C,

if the net rate of formation of B is set to be zero then the concentration of B is given by:

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

For an elementary chemical reaction, $A_{2} ⇄_{k_{- 1}}^{k_{1}} 2 A$ , the expression for $\frac{d [A]}{dt}$ is:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

The rate of chemical reaction doubles for every

100

rise in temperature. If the temperature increase by

600,

the rate of reaction increases

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

A + 2 B \to C

, the rate equation for the reaction is given as

Rate

= k [A] [B]

If the concentration of A is kept the same but that of B is doubled what will happen to the rate itself?

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

Mechanism of a hypothetical reaction

X_{2} + Y_{2} \to 2 XY

is given below:

(i)

X_{2} \to X + X (fast)

(ii)

X + Y_{2} ⇌ XY + Y (slow)

(iii)

X + Y \to XY (fast)

The overall order of the reaction will be

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

Find the unit of the rate constant of a reaction represented with a rate equation, rate

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

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

For an elementary reaction

2 A + 3 B \to 4 C + D

the rate of appearance of

C

at time

' t'

2.8 \times 10^{- 3} mol L^{- 1} S^{- 1}

. Rate of disappearance of

B

' t'

t

will be

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

For the chemical reaction

N_{2} (g) + 3 H_{2} (g) ⇋ 2 N H_{3} (g)

, the correct option is:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Rate of a Chemical Reaction

For the reaction,

3A + 2B \to C + D

, the differential rate law can be written as :

For a reaction dxdt=KH+n. If pH of the reaction medium changes from two to one the rate becomes 100 times of value at pH=2. What is the order of reaction?

Important Questions on Chemical Kinetics

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For a reaction $\frac{d x}{d t} = K {[H^{+}]}^{n}$ . If $p H$ of the reaction medium changes from two to one the rate becomes $100 t i m e s$ of value at $p H = 2$ . What is the order of reaction?