Find the molecularity of the reaction, Cl → 1 2 Cl 2 ( g ) . Give the potential energy diagram to explain activation energy.

Molecularity is defined as the number of reactants taking part in a chemical reaction. For the given reaction, Cl → 1 2 Cl 2 ( g ) , molecularity is one. Activation energy is required by reactants to form activated complexes and is equal to the difference between threshold energy and average kinetic energy. This can be explained by the following graph :

Find the molecularity of the reaction, Cl → 1 2 Cl 2 ( g ) . Give the potential energy diagram to explain activation energy.

Molecularity is defined as the number of reactants taking part in a chemical reaction. For the given reaction, Cl → 1 2 Cl 2 ( g ) , molecularity is one. Activation energy is required by reactants to form activated complexes and is equal to the difference between threshold energy and average kinetic energy. This can be explained by the following graph :

The data given is for the reaction, N 2 O 5 g → NO 2 g + O 2 g : S.no. N 2 O 5 ( mol L - 1 ) Rate of disappearance of N 2 O 5 mol L - 1 min - 1 1 1 . 13 × 10 - 2 34 × 10 - 5 2 0 . 84 × 10 - 2 25 × 10 - 5 3 0 . 62 × 10 - 2 18 × 10 - 5 Determine the order of reaction.

Rate law expression for the reaction can be given as : Rate = k N 2 O 5 x . Where, x is the order of the reaction. 25 × 10 - 5 = k 0 . 84 × 10 - 2 x 18 × 10 - 5 = k 0 . 62 × 10 - 2 x 25 × 10 - 5 18 × 10 - 5 = k 0 . 84 × 10 - 2 x k 0 . 62 × 10 - 2 x 1 . 38 = 1 . 36 x x = 1 The order of reaction comes out to be one. Hence, the given reaction is of first order.

The data given is for the reaction, N 2 O 5 g → NO 2 g + O 2 g : S.no. N 2 O 5 ( mol L - 1 ) Rate of disappearance of N 2 O 5 mol L - 1 min - 1 1 1 . 13 × 10 - 2 34 × 10 - 5 2 0 . 84 × 10 - 2 25 × 10 - 5 3 0 . 62 × 10 - 2 18 × 10 - 5 Determine the rate law of reaction.

Rate law expression for the reaction can be given as : Rate = k N 2 O 5 x , where k is rate constant. 25 × 10 - 5 = k 0 . 84 × 10 - 2 x 18 × 10 - 5 = k 0 . 62 × 10 - 2 x 25 × 10 - 5 18 × 10 - 5 = k 0 . 84 × 10 - 2 x k 0 . 62 × 10 - 2 x 1 . 38 = 1 . 36 x x = 1 Rate law for the reaction can be given as : Rate = k N 2 O 5 .

Under what condition a bimolecular reaction behaves kinetically first order reaction?

In a bimolecular reaction, when the amount of one of the reactants is present in excess, the reaction is kinetically first order because the concentration of reactant present in excess does not affect the order of reaction. Hence, it does not affect the rate of reaction and such reactions are called pseudo first order reactions. Example : Hydrolysis of sucrose yielding glucose and fructose.

E M B I B E

All In One ISC Chemistry Class 12>Chapter 4 - Chemical Kinetics>Chapter Practice>Q 24

HARD

12th ICSE

IMPORTANT

Earn 100

Find the molecularity of the reaction, $Cl \to \frac{1}{2} {Cl}_{2} (g)$ . Give the potential energy diagram to explain activation energy.

Important Questions on Chemical Kinetics

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12th ICSE

IMPORTANT

All In One ISC Chemistry Class 12>Chapter 4 - Chemical Kinetics>Chapter Practice>Q 25

State the role of activated complex in a reaction and state its relation with activation energy.

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IMPORTANT

All In One ISC Chemistry Class 12>Chapter 4 - Chemical Kinetics>Chapter Practice>Q 26

Illustrate graphically the effect of catalyst on activation energy.

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IMPORTANT

All In One ISC Chemistry Class 12>Chapter 4 - Chemical Kinetics>Chapter Practice>Q 26

Catalysts have no effect on the equilibrium constant, why?

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IMPORTANT

All In One ISC Chemistry Class 12>Chapter 4 - Chemical Kinetics>Chapter Practice>Q 27

The rate of a chemical reaction doubles for every

10 ° C

rise in temperature. If the temperature is raised from

10 ° C

to

30 ° C

, what will be the increase in the rate of the reaction?

HARD

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IMPORTANT

All In One ISC Chemistry Class 12>Chapter 4 - Chemical Kinetics>Chapter Practice>Q 28

The activation energy of a reaction is

94.14 kJ {mol}^{- 1}

and the value of rate constant at

298 K

is

18 x 10^{- 5} s^{- 1}

. Calculate the frequency factor or pre-exponential factor,

A

.

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IMPORTANT

All In One ISC Chemistry Class 12>Chapter 4 - Chemical Kinetics>Chapter Practice>Q 29

For a reaction, the energy of activation is zero. What is the value of rate constant at

300 K

, if

k = 1.6 x 10^{6} s^{- 1}

at

280 K

?

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IMPORTANT

All In One ISC Chemistry Class 12>Chapter 4 - Chemical Kinetics>Chapter Practice>Q 30

The data given is for the reaction, $N_{2} O_{5} (g) \to {NO}_{2} (g) + O_{2} (g)$ :

S.no.	$N_{2} O_{5} (mol L^{- 1})$	Rate of disappearance of $N_{2} O_{5}$ $(mol L^{- 1} \min^{- 1})$
$1$	$1.13 \times 10^{- 2}$	$34 \times 10^{- 5}$
$2$	$0.84 \times 10^{- 2}$	$25 \times 10^{- 5}$
$3$	$0.62 \times 10^{- 2}$	$18 \times 10^{- 5}$

Determine the order of reaction.

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IMPORTANT

All In One ISC Chemistry Class 12>Chapter 4 - Chemical Kinetics>Chapter Practice>Q 30

The data given is for the reaction, $N_{2} O_{5} (g) \to {NO}_{2} (g) + O_{2} (g)$ :

S.no.	$N_{2} O_{5} (mol L^{- 1})$	Rate of disappearance of $N_{2} O_{5}$ $(mol L^{- 1} \min^{- 1})$
$1$	$1.13 \times 10^{- 2}$	$34 \times 10^{- 5}$
$2$	$0.84 \times 10^{- 2}$	$25 \times 10^{- 5}$
$3$	$0.62 \times 10^{- 2}$	$18 \times 10^{- 5}$