For reaction R → P , in 25 minutes the concentration of reactant changed from 0 . 03 M to 0 . 02 M . Give the average velocity in seconds and minutes.

The average velocity of the reaction is given by: V _ = - ∆ C ∆ t , where ∆ C , ∆ t are change in concentrations from reactants to products and change in time respectively. Given, ∆ t = 25 mins = 1500 s , C 2 = 0 . 02 M , C 1 = 0 . 03 M Substituting in the equation we get: V _ = C 1 - C 2 ∆ t = 0 . 03 - 0 . 02 25 = 4 × 10 - 4 M min - 1 In terms of seconds the average velocity is = 4 × 10 - 4 60 = 6 . 67 × 10 - 6 M sec - 1

In a reaction 2 A → Product . Initial concentration is 0 . 5 mol L - 1 which reduced upto 0 . 4 mol L - 1 in 10 minutes. Calculate the rate of reaction for this time period.

For the reaction 2 A → Product The rate of the reaction is given by: Rate = - 1 2 ∆ A ∆ t , where ∆ A , ∆ t are change in concentration of reactant and change in time respectively. Given, ∆ t = 10 mins , A 2 = 0 . 4 M , A 1 = 0 . 5 M Substituting in the equation we get: Reaction rate = - 1 2 A 2 - A 1 ∆ t = - 1 2 0 . 4 - 0 . 5 10 = 5 × 10 - 3 M min - 1 In terms of seconds the rate of reaction is 8 . 33 × 10 - 5 M sec - 1 .

What is the order for the following reactions? 2 NO 2 ( g ) + F 2 ( g ) → 2 NO 2 F ( g ) , rate= k [ NO 2 ] [ F 2 ]

Rate Law is defined as the law which is used for studying the relationship between the rate of reaction and the concentration of the reactants. 2 NO 2 ( g ) + F 2 ( g ) ⟶ 2 NO 2 F ( g ) rate = k [ NO 2 ] [ F 2 ] The rate law shows that the reaction is first order with respect to NO 2 and first order with respect to F 2 . Hence overall order of reaction is, 1 + 1 = 2 .

For the chemical reaction N 2 g + 3 H 2 g ⇋ 2 N H 3 g , the correct option is:

- d [ N 2 ] d t = 1 2 d [ N H 3 ] d t

- 1 3 d [ H 2 ] d t = - 1 2 d [ N H 3 ] d t

- d [ N 2 ] d t = 2 d [ N H 3 ] d t

3 d [ H 2 ] d t = 2 d [ N H 3 ] d t

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IMPORTANT

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Graph of half life of zero-order reaction and initial concentration of reactant is a (straight line/parabola).

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Important Questions on Chemical Kinetics

EASY

12th ICSE

IMPORTANT

Chemistry Crash Course (Based on Revised Syllabus-2023)>Chapter 1 - Chemical Kinetics>Exercise>Q 11

Why does the rate of any reaction generally decreases during the course of the reaction?

MEDIUM

12th ICSE

IMPORTANT

Chemistry Crash Course (Based on Revised Syllabus-2023)>Chapter 1 - Chemical Kinetics>Exercise>Q 12

For reaction

R \to P

, in

25

minutes the concentration of reactant changed from

0.03 M

0.02 M

. Give the average velocity in seconds and minutes.

MEDIUM

12th ICSE

IMPORTANT

Chemistry Crash Course (Based on Revised Syllabus-2023)>Chapter 1 - Chemical Kinetics>Exercise>Q 13

In a reaction

2 A \to Product

. Initial concentration is

0.5 mol L^{- 1}

which reduced upto

0.4 mol L^{- 1}

10

minutes. Calculate the rate of reaction for this time period.

HARD

12th ICSE

IMPORTANT

Chemistry Crash Course (Based on Revised Syllabus-2023)>Chapter 1 - Chemical Kinetics>Exercise>Q 14

For the reaction- $2 A + B \to A_{2} B,$

The rate $= k [A] [B]^{2}$ with $k = 2.0 \times 10^{- 6} {mol}^{- 2} L^{2} s^{- 1}$ . Calculate the initial rate of reaction when $[A] = 0.1 mol L^{- 1}$ , $[B] = 0.2 mol L^{- 1}$ . Calculate the rate of reaction after $[A]$ is reduced to $0.06 mol L^{- 1}$ .

HARD

12th ICSE

IMPORTANT

Chemistry Crash Course (Based on Revised Syllabus-2023)>Chapter 1 - Chemical Kinetics>Exercise>Q 15

The decomposition of

{NH}_{3}

on platinum surface is zero order reaction. What are the rates of production of

N_{2}

and

H_{2}

. If

k = 2.5 \times 10^{- 4} mol L^{- 1} \sec^{- 1}

EASY

12th ICSE

IMPORTANT

Chemistry Crash Course (Based on Revised Syllabus-2023)>Chapter 1 - Chemical Kinetics>Exercise>Q 16

What is the order for the following reactions?

2 {NO}_{2} (g) + F_{2} (g) \to 2 {NO}_{2} F (g),

rate=

k [{NO}_{2}] [F_{2}]

EASY

12th ICSE

IMPORTANT

Chemistry Crash Course (Based on Revised Syllabus-2023)>Chapter 1 - Chemical Kinetics>Exercise>Q 17

The rate law for the reaction

C_{2} H_{4} {Br}_{2} + 3 I^{-} \to C_{2} H_{4} + 2 {Br}^{-} + I_{3}^{-}

is rate

= k [C_{2} H_{4} {Br}_{2}] [I^{- 1}]

. The rate of the reaction is found to be

1.1 x 10^{- 4} M / s

when the concentrations of

C_{2} H_{4} {Br}_{2}

and

I^{-}

are

0.12 M

and

0.18 M

respectively. Calculate the rate constant of the reaction,

HARD

12th ICSE

IMPORTANT

Chemistry Crash Course (Based on Revised Syllabus-2023)>Chapter 1 - Chemical Kinetics>Exercise>Q 18

Consider the reaction

C + D \to

products. The rate of the reaction increases by a factor of

4

when concentration of

C

is doubled. The rate of the reaction is tripled when concentration of

D

is tripled. What is the order of the reaction? Write the rate law.

Graph of half life of zero-order reaction and initial concentration of reactant is a (straight line/parabola).

Important Questions on Chemical Kinetics

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