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For a hypothetical elementary reaction.

where $\frac{k_{1}}{k_{2}} = \frac{1}{2}$

Initially, only $2$ moles of $A$ are present. The total number of moles of $A, B$ and $C$ at the end of $75 %$ of reaction are:

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Important Questions on Chemical Kinetics

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-1>Q 70

The rate constant, the activiation energy and the Arrhenius parameter of a chemical reaction at

25 ° C

are

3.0 \times 10^{- 4} s^{- 1}

104.4 kJ {mol}^{- 1}

and

6.0 \times 10^{14} s^{- 1}

, respectively. The value of the rate constant at

T \to \infty

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-1>Q 71

The rate constant

K_{1}

of a reaction is found to be double that of the rate constant

K_{2}

of another reaction. The relationship between corresponding activation energies of the two reactions at the same temperature

(E_{1} and E_{2})

can be represented as:

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-1>Q 73

How much faster would a reaction proceed at

25 ° C

than at

0 ° C

, if the activation energy is

65 kJ

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-1>Q 77

For the reaction,

H_{2} (g) + {Br}_{2} (g) \to 2 HBr (g)

, the experiment data suggested that

r = k [H_{2}] {[{Br}_{2}]}^{1 / 2}

. The molecularity and order of the reaction are, respectively:

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-1>Q 78

The reaction of ${NO}_{2} (g)$ and $O_{3} (g)$ is first order in ${NO}_{2} (g)$ and $O_{3} (g)$

$2 {NO}_{2} (g) + O_{3} (g) ⟶ N_{2} O_{5} (g) + O_{2} (g)$

The reaction can take place by mechanism:

$I : {NO}_{2} + O_{3} \overset{sbw}{⟶} {NO}_{3} + O_{2}$

${NO}_{3} + {NO}_{2} \overset{fast}{⟶} N_{2} O_{5}$

$II : O_{3} ⇌_{K_{b}}^{k_{a} fast} O_{2} + [O]$

${NO}_{2} + O \overset{slow}{⟶} {NO}_{3}$

${NO}_{3} + {NO}_{2} \overset{fast}{⟶} N_{2} O_{5}$

Select correct mechanism.

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-1>Q 80

The reaction of hydrogen and iodine monochloride is represented by the equation:

$H_{2} (g) + 2 ICl (g) ⟶ 2 HCl (g) + I_{2} (g)$

This reaction is first-order in $H_{2} (g)$ and also first-order in $ICl (g)$ . Which of these proposed mechanisms can be consistent with the given information about this reaction?

Mechanism $I$ : $H_{2} (g) + 2 ICl (g) ⟶ 2 HCl (g) + I_{2} (g)$

Mechanism $II$ : $H_{2} (g) + ICl (g) \overset{Slow}{⟶} HCl (g) + HI (g)$

$Hl (g) + ICl (g) \overset{fast}{⟶} HCl (g) + I_{2} (g)$

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-1>Q 82

A radioactive element has a half-life of one day. After three days the amount of the element left will be:

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-1>Q 83

A sample of rock from the moon contains equal number of atoms of uranium and lead

(t_{\frac{1}{2}} for U = 4.5 \times 10^{9} years)

. The age of the rock would be:

For a hypothetical elementary reaction. where k1k2=12 Initially, only 2 moles of A are present. The total number of moles of A, B and C at the end of 75% of reaction are:

Important Questions on Chemical Kinetics

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For a hypothetical elementary reaction.

where $\frac{k_{1}}{k_{2}} = \frac{1}{2}$

Initially, only $2$ moles of $A$ are present. The total number of moles of $A, B$ and $C$ at the end of $75 %$ of reaction are: