For the reaction, 2 A + B → products, when the concentration of A and B both were doubled, the rate of the reaction increased from 0.3 m o l L - 1 s - 1 to 2.4 m o l L - 1 s - 1 . When the concentration of A alone is doubled, the rate increased from 0.3 m o l L - 1 s - 1 to 0.6 m o l L - 1 s - 1 . Which one of the following statements is correct?

Order of the reaction with respect to B is 2

Total order of the reaction is 4

Order of the reaction with respect to A is 2

Order of the reaction with respect to B is 1

EASY

Earn 100

A substance undergoes first order decomposition. The decomposition follows two parallel first order reactions as:

$k_{1} = 1.26 \times 1 0^{- 4} s^{-1}$ , $k_{2} = 3.8 \times 1 0^{- 5} s^{-1}$

The percentage distribution of $B and C$ are

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Important Questions on Chemical Kinetics

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

Consider the following reversible reaction:

A (g) + B (g) ⇌ AB (g)

The activation energy of the backward reaction exceeds that of the forward reaction by

2 RT

(in

{mol}^{- 1}

). If the pre-exponential factor of the forward reaction is

4

times that of the reverse reaction, the absolute value of

∆ G^{⊝} (in J {mol}^{- 1})

for the reaction at

300 K

is ____.

(Given;

\ln (2) = 0 .7, = 2500 J {mol}^{- 1} at 300 K

and

G

is the Gibbs energy)

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

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

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

For a first order reaction

A (g) \to 2 B (g) + C (g)

at constant volume and 300 K, the total pressure at the beginning

(t = 0)

and at time are

p_{0} and p_{t}

, respectively. Initially, only A is present with concentration

{[A]}_{0}

, and

t_{\frac{1}{3}}

is the time required for the partial pressure of A to reach

1 / 3^{rd}

of its initial value. The correct option(s) is (are)
(Assume that all these gases behave as ideal gases)

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

The reaction

2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)

follows first order kinetics. The pressure of a vessel containing only

N_{2} O_{5}

was found to increase from 50 mm Hg to 87.5 mm Hg in 30 min. The pressure exerted by the gases after 60 min. Will be (Assume temperature remains constant) :

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

The rate of a first-order reaction is

0.04 m o l l^{- 1} s^{- 1}

10

second and

0.03 m o l l^{- 1} s^{- 1}

20

seconds after initiation of the reaction. The half-life period of the reaction is:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

The rate of a reaction doubles when its temperature changes from

300 K to 310 K

. Activation energy of such a reaction will be:

(R = {8.314 JK}^{-1} {mol}^{-1} and log 2 = 0.301)

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

For a reaction, consider the plot of $l n k$ versus $1 / T$ given in the figure. If the rate constant of this reaction at $400 K$ is $10^{- 5} s^{- 1}$ , then the rate constant at $500 K$ is:

Question Image

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

A reaction has an activation energy of

209 k J m o l^{- 1}

. The rate increases

10

-fold when the temperature is increased from

27^{o} C

X^{o} C

. The temperature

X

is closest to

[Gas constant,

R = 8.314 J m o l^{- 1} K^{- 1}

]

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

Consider the given plots for a reaction obeying Arrhenius equation $(0 ° C < T < 300 ° C) :$ ( $K$ and $E_{a}$ are rate constant and activation energy, respectively )

(I)

Question Image

(II)

Question Image

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

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

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

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?

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

According to the Arrhenius equation,

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

For the equilibrium,

A (g) ⇌ B (g), ∆ H is - 40 kJ / mol

. If the ratio of the activation energies of the forward

(E_{f})

and reverse

(E_{b})

reactions is

\frac{2}{3}

then:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

The rate constant of the reaction

A ⟶ B

0.6 \times 10^{- 3}

mole per liter per second. If the initial concentration of A is 5 M, then the concentration of B after 20 minutes is:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

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

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

The enthalpy

(H)

of an elementary exothermic reaction

A ⇌ B

is schematically plotted against the reaction coordinate. The plots in the presence and absence of a catalyst are shown in dashed and solid lines, respectively. Identify the correct plot for the reaction.

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

For the reaction,

2 A + B \to

products, when the concentration of

A

and

B

both were doubled, the rate of the reaction increased from

0.3 m o l L^{- 1} s^{- 1}

2.4 m o l L^{- 1} s^{- 1} .

When the concentration of

A

alone is doubled, the rate increased from

0.3 m o l L^{- 1} s^{- 1}

0.6 m o l L^{- 1} s^{- 1} .

Which one of the following statements is correct?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

The addition of a catalyst during a chemical reaction alters which of the following quantities?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Law for Zero and First Order Reactions

For

n^{th}

order of reaction, Half-life period is directly proportional to

A substance undergoes first order decomposition. The decomposition follows two parallel first order reactions as: k 1 = 1.26 × 1 0 - 4 s -1 , k 2 = 3.8 × 1 0 - 5 s -1 The percentage distribution of B and C are

Important Questions on Chemical Kinetics

Learn and Prepare for any exam you want !

A substance undergoes first order decomposition. The decomposition follows two parallel first order reactions as:

$k_{1} = 1.26 \times 1 0^{- 4} s^{-1}$ , $k_{2} = 3.8 \times 1 0^{- 5} s^{-1}$

The percentage distribution of $B and C$ are