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

HARD

Earn 100

A reaction $X_{2} (g) \to Z (g) + \frac{1}{2} Y (g)$ exhibits an increase in pressure from 150 mm to 170 mm in 10 minutes. The rate of disappearance of $X_{2}$ in mm per minute is

50% studentsanswered this correctly

Important Questions on Redox Reactions and Rate of Chemical Reactions

MEDIUM

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of Chemical Reaction

For the reaction

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

, which statement is correct?

MEDIUM

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of Chemical Reaction

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

EASY

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of 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

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of Chemical Reaction

For the chemical reaction

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

, the correct option is:

EASY

Science>Chemistry>Redox Reactions and Rate of Chemical Reactions>Rate of Chemical Reaction

For the reaction,

3A + 2B \to C + D

, the differential rate law can be written as :

A reaction X2(g)→Z(g)+12Y(g) exhibits an increase in pressure from 150 mm to 170 mm in 10 minutes. The rate of disappearance of X2 in mm per minute is

Important Questions on Redox Reactions and Rate of Chemical Reactions

Learn and Prepare for any exam you want !

A reaction $X_{2} (g) \to Z (g) + \frac{1}{2} Y (g)$ exhibits an increase in pressure from 150 mm to 170 mm in 10 minutes. The rate of disappearance of $X_{2}$ in mm per minute is