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For a ﬁrst order reaction, $A \to P, t_{\frac{1}{2}}$ (half-life) is $10$ days. The time required for $\frac{1^{t h}}{4}$ conversion of $A$ (in days) is: $(\ln 2 = 0.693, \ln 3 = 1.1)$

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Important Questions on Chemical Kinetics

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-3>Q 68

If 50 % of a reaction occurs in 100 second and 75 % of the reaction occurs in 200 second, the order of this reaction is:

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-3>Q 69

The following results were obtained during kinetic studies of the reaction

2 A + B \to

Products

Experiment	$[A]$ in $(mol L^{- 1})$	$[B]$ (in $mol L^{- 1}$ )	Initial Rate of reaction (in $mol L^{- 1} \min^{- 1}$ )
(I)	$0.10$	$0.20$	$6.93 \times 10^{- 3}$
(II)	$0.10$	$0.25$	$6.93 \times 10^{- 3}$
(III)	$0.20$	$0.30$	$1.386 \times 10^{- 2}$

The time (in minutes) required to consume half of $A$ is

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-3>Q 71

For an elementary chemical reaction,

$A_{2} ⇌_{K_{- 1}}^{K_{1}} 2 A$ the expressions for $\frac{d [A]}{dt}$

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-3>Q 72

If a reaction follows the Arrhenius equation, the plot

lnk

\frac{1}{(RT)}

gives straight line with a gradient

(- y)

unit. The energy required to activate the reactant is:

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-3>Q 74

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

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-4>Q 1

Which energy diagram corresponds to exothermic reaction and highest value of the rate constant?

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-4>Q 2

The experimental observations for the following reaction are given below:
$P + Q \to$ Product.

$[P] / M$	$[Q] / M$	Initial Rate $/ {mols}^{- 1}$
$0.2$	$0.5$	$8 \times 10^{- 3}$
$0.4$	$0.5$	$3.2 \times 10^{- 2}$
$0.2$	$0.25$	$4 \times 10^{- 3}$

The order of this reaction is:

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Alpha Question Bank for Engineering: Chemistry>Chapter 10 - Chemical Kinetics>Exercise-4>Q 3

The reaction

A (g) + 2 B (g) ⟶ C (g)

is an elementary reaction. In an experiment involving this reaction, the initial partial pressures of

A

and

B

are

P_{A} = 0.40

atm and

P_{B} = 1.0

atm respectively. When

P_{C} = 0.3

atm, the rate of the reaction relative to the initial rate is:

For a ﬁrst order reaction, A→P, t12 (half-life) is 10 days. The time required for 1th4 conversion of A (in days) is: ln⁡2=0.693,ln⁡3=1.1

Important Questions on Chemical Kinetics

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For a ﬁrst order reaction, $A \to P, t_{\frac{1}{2}}$ (half-life) is $10$ days. The time required for $\frac{1^{t h}}{4}$ conversion of $A$ (in days) is: $(\ln 2 = 0.693, \ln 3 = 1.1)$