A zero order reaction is a multi-step reaction

A second order reaction is always a multistep reaction

A first order reaction is always a single step reaction

A zero order reaction is a single step reaction

Under what condition the order of the reaction, 2 H I → H 2 g + I 2 g , is zero

At high partial pressure of H I

At high partial pressure of H 2

At high partial pressure of I 2

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For a second order reaction, $2 A \to$ Products, a plot of log $t_{1 / 2} vs \log a$ (where, $a$ is initial concentration) will give an intercept equal to

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Important Questions on Chemical Kinetics

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Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The rate constant for the first order reaction is

60 s^{- 1} .

How much time will it take to reduce the concentration of the reactant to

\frac{1}{16} t h

value?

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For a zero - order reaction with rate constant k, the slope of the plot reactant concentration against time is

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The half-life period of a first-order reaction is

15 minutes

. The amount of substance left after one hour will be

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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

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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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The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i) and (ii)$ . The respective orders of the reaction are
(i) Question Image

(ii) Question Image

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A first-order reaction has a specific reaction rate

10^{- 2} \sec^{- 1} .

How much time will it take for

20 g

the reactant to reduce to

5 g

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A flask contains a mixture of compounds

A

and

B

. Both compounds decompose by first-order kinetics. The half-lives for

A

and

B

are

300 s

and

180 s

, respectively. If the concentrations of

A

and

B

are equal initially, the time required for the concentration of A to be four times that of

B

(in s) is :

(Use \ln 2 = 0.693)

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It takes

1 h

for a first order reaction to go to

50 %

completion. The total time required for the same reaction to reach

87.5 %

completion will be

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Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The rate constant for a first order reaction is

7 .0 \times 10^{- 4} s^{- 1} .

If initial concentration of the reactant is

0.080 M

, what is the half-life of the reaction?

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Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

If the rate constant for a first order reaction is

k

, the time

(t)

required for the completion of

99 %

of the reaction is given by

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

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) :

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The rate constant of a first order reaction is

231 \times 10^{- 5} s^{- 1}

. How long will

4 g

of this reactant reduce to

2 g

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Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

Decomposition of

H_{2} O_{2}

follows a first order reaction. In fifty minutes the concentration of

H_{2} O_{2}

decreases from

0.5

0.125 M

in one such decomposition. When the concentration of

H_{2} O_{2}

reaches

0.05 M

, the rate of formation of

O_{2}

will be:

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Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

It is true that:

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Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

The half-life for a zero order reaction having

0.02 M

initial concentration of reactant is

100 s

. The rate constant (in

mol L^{- 1} s^{- 1}

) for the reaction is

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The rate constant for a first order reaction is

4.606 \times 10^{- 3} s^{- 1}

. The time required to reduce

2.0 g

of the reactant to

0.2 g

is :

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Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

Under what condition the order of the reaction,

2 H I \to H_{2} (g) + I_{2} (g),

is zero

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Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

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

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Chemistry>Physical Chemistry>Chemical Kinetics>Integrated Rate Equations of Chemical Reaction

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:

For a second order reaction, 2A→ Products, a plot of log t1/2 vs log a (where, a is initial concentration) will give an intercept equal to

Important Questions on Chemical Kinetics

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For a second order reaction, $2 A \to$ Products, a plot of log $t_{1 / 2} vs \log a$ (where, $a$ is initial concentration) will give an intercept equal to