Question Bank for NEET Chemistry Chemical Kinetics / रासायनिक बलगतिकी Self Evaluation Test - Chemical Kinetics

\[{{N}_{2}}{{O}_{5}}(g)\xrightarrow{{}}2N{{O}_{2}}(g)+1/2\,{{O}_{2}}(g)\] the value of rate of disappearance of \[{{N}_{2}}{{O}_{5}}\] is given as \[6.25\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]. The rate of formation of \[N{{O}_{2}}\] and \[{{O}_{2}}\] is given respectively as:

A)

\[6.25\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\] and \[6.25\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\]

B)

\[1.25\times {{10}^{-2}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\] and \[3.125\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\]

C)

\[6.25\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\] and \[3.125\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\]

D)

\[1.125\times {{10}^{-2}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\]and \[6.25\times {{10}^{-3}}mol\text{ }{{L}^{-1}}{{s}^{-1}}\]

View Solution

2)

The reactions rate \[{{N}_{2}}\left( g \right)+3{{H}_{2}}\left( g \right)\to 2N{{H}_{3}}\left( g \right)\]was measured\[\frac{d[N{{H}_{3}}]}{dt}=2\times {{10}^{-4}}mol\,{{\sec }^{-1}}\]. The rates of reactions expressed in terms of \[{{N}_{2}}\]and \[{{H}_{2}}\] are

A)

Rate in terms of \[{{N}_{2}}\] \[(mol\,{{L}^{-1}}se{{c}^{-1}})\]	Rate in terms of \[{{H}_{2}}\] \[(mol\,{{L}^{-1}}se{{c}^{-1}})\]
\[2\times {{10}^{-4}}\]	\[2\times {{10}^{-4}}\]

B)

Rate in terms of \[{{N}_{2}}\] \[(mol\,{{L}^{-1}}se{{c}^{-1}})\]	Rate in terms of \[{{H}_{2}}\] \[(mol\,{{L}^{-1}}se{{c}^{-1}})\]
\[3\times {{10}^{-4}}\]	\[1\times {{10}^{-4}}\]

C)

Rate in terms of \[{{N}_{2}}\] \[(mol\,{{L}^{-1}}se{{c}^{-1}})\]	Rate in terms of \[{{H}_{2}}\] \[(mol\,{{L}^{-1}}se{{c}^{-1}})\]
\[1\times {{10}^{-4}}\]	\[3\times {{10}^{-4}}\]

D)

Rate in terms of \[{{N}_{2}}\] \[(mol\,{{L}^{-1}}se{{c}^{-1}})\]	Rate in terms of \[{{H}_{2}}\] \[(mol\,{{L}^{-1}}se{{c}^{-1}})\]
\[2\times {{10}^{-1}}\]	\[2\times {{10}^{-3}}\]

View Solution

3)

For the reaction\[A+B\xrightarrow{{}}C+D\]. The variation of the concentration of the products is given by the curve

A)

Z

B)

Y

C)

W

D)

X

View Solution

4)

For the reaction \[{{H}_{2}}\left( g \right)+B{{r}_{2}}\left( g \right)\to 2HBr\left( g \right),\] the experimental data suggest, rate\[=k[{{H}_{2}}]{{[B{{r}_{2}}]}^{1/2}}\]. The molecularity and order of the reaction are respectively

A)

\[2,\frac{3}{2}\]

B)

\[\frac{3}{2},\frac{3}{2}\]

C)

1,1

D)

\[1,\frac{1}{2}\]

View Solution

5)

For a chemical reaction \[{{t}_{1/2}}\] is 2.5 hours at room temperature. How much of the reactant will be left after 7.5 hours if initial weight of reactant was 160g?

A)

10 g

B)

40 g

C)

80 g

D)

20 g

View Solution

6)

The rate law for a reaction between the substances A and B is given by rate \[=k{{[A]}^{n}}{{[B]}^{m}}\] On doubling the concentration of A and halving the concentration of B, the ratio of the new rate to the earlier rate of the reaction will be as

A)

\[\left( m+n \right)\]

B)

\[\left( n-m \right)\]

C)

\[{{2}^{\left( n+m \right)}}\]

D)

\[\frac{1}{{{2}^{\left( m+n \right)}}}\]

View Solution

7)

The order of a reaction, with respect to one of the reacting component Y, is zero. It implies that:

A)

the reaction is going on at a constant rate

B)

the rate of reaction does not vary with temperature

C)

the reaction rate is independent of the concentration of Y

D)

the rate of formation of the activated complex is zero

View Solution

8)

For a first order reaction, a plot of log \[\left( a-x \right)\] against time is a straight line with a negative slope equal to

A)

\[\frac{-k}{2.303}\]

B)

\[-2.303k\]

C)

\[\frac{2.303}{k}\]

D)

\[-\frac{{{E}_{a}}}{2.303R}\]

View Solution

9)

A following mechanism has been proposed for a reaction

\[2A+B\to D+E\]

\[A+B\to C+D\left( slow \right)\]

\[A+C\to E\left( fast \right)\]

The rate law expression for the reaction is:

A)

\[r=k{{\left[ A \right]}^{2}}\left[ B \right]\]

B)

\[r=k\left[ A \right]\left[ B \right]\]

C)

\[r=k{{\left[ A \right]}^{2}}\]

D)

\[r=k\left[ A \right]\left[ C \right]\]

View Solution

10)

The rate law for the reaction below is given by the expression k [A] [B] \[A+B\to Product\] If the concentration of B is increased from 0.1 to 0.3 mole, keeping the value of A at 0.1 mole, the rate constant will be:

A)

3k

B)

9k

C)

k/3

D)

k

View Solution

11)

The half-life of a radioactive element is 20 min. The time interval between the stages of its 33% and 67% decay is

A)

40 min

B)

20 min

C)

30min

D)

25 min

View Solution

12)

Which of the following reactions is not of the first order?

A)

Inversion of sucrose in the presence of acid

B)

Acid-catalyzed hydrolysis of ethyl acetate

C)

Hydrolysis of tertiary butyl halide using alkali

D)

Oxidation of \[{{I}^{-}}\] ion by \[{{S}_{2}}O_{8}^{2-}\] ion

View Solution

13)

Rate constant \[k=1.2\times {{10}^{3}}mo{{l}^{-1}}\,L\,{{s}^{-1}}\]and \[{{E}_{a}}=2.0\times {{10}^{2}}\,kJ\,mo{{l}^{-1}}\] When \[T\to \infty :\]

A)

\[A=2.0\times {{10}^{2}}kJ\,mo{{l}^{-1}}\]

B)

\[A=1.2\times {{10}^{3}}\,mo{{l}^{-1}}L\,{{S}^{-1}}\]

C)

\[A=1.2\times {{10}^{3}}mol\,{{L}^{-1}}{{s}^{-1}}\]

D)

\[A=2.4\times {{10}^{3}}kJ\,mo{{l}^{-1}}{{s}^{-1}}\]

View Solution

14)

A catalyst lowers the activation enegy of a reaction from \[20kJ\text{ }mo{{l}^{-1}}\] to\[10kJ\text{ }mo{{l}^{-1}}\]. The temperature at which the uncatalyzed reaction will have the same rate as that of the catalyzed at \[27{}^\circ C\] is

A)

\[-123{}^\circ C\]

B)

\[327{}^\circ C\]

C)

\[32.7{}^\circ C\]

D)

\[+23{}^\circ C\]

View Solution

15)

For a reaction, the rate constant is expressed as\[k=A{{e}^{-40000/T}}\]. The energy of the activation is

A)

40000 cal

B)

88000 cal

C)

80000 cal

D)

8000 cal

View Solution

16)

The activation energy of the reaction, \[A+B\to C+D+38\] kcal is 20 kcal. What would be the activation energy of the following reaction \[C+D\to A+B\]

A)

20 kcal

B)

-20 kcal

C)

18 kcal

D)

58 kcal

View Solution

17)

The half-life of a reaction is inversely proportional to the square of the initial concentration of the reactant. Then the order of the reaction is

A)

0

B)

1

C)

2

D)

3

View Solution

18)

For a reaction\[A+2B\to C\], the amount of C formed by starting the reaction with 5 moles of A and 8 moles of B is

A)

5 moles

B)

8 moles

C)

16 moles

D)

4 moles

View Solution

19)

The rate law for the reaction \[2X+Y\to Z\] is Rate \[=k\left[ X \right]\left[ Y \right].\] The correct statement with regard to this relation is

A)

the unit of k is \[{{s}^{-1}}\]

B)

the rate of the reaction is independent of [X] and [Y]

C)

for this reaction \[{{t}_{1/2}}\] is independent of initial concentrations of reactant

D)

the rate of formation of Z is half of the rate of disappearance of X

View Solution

20)

In a reaction, \[2A\to \] products, the concentration of A decreases from 0.50 M to 0.38 M in 10 min. What is the rate of reaction (in\[M\text{ }{{s}^{-1}}\]) during this interval?

A)

0.012

B)

0.024

C)

\[2\times {{10}^{-3}}\]

D)

\[2\times {{10}^{-4}}\]

View Solution

21)

A chemical reaction is catalyzed by a catalyst X. Hence X

A)

reduces enthalpy of the reaction

B)

decreases rate constant of the reaction

C)

increases activation energy of the reaction

D)

does not affect equilibrium constant of the reaction

View Solution

22)

In respect of the equation \[k=A{{e}^{-Ea/RT}}\] in chemical kinetics, which one of the following statements is correct?

A)

A is adsorption factor

B)

\[{{E}_{a}}\]is energy of activation

C)

R is Rydberg's constant

D)

k is equilibrium constant

View Solution

23)

The minimum energy a molecule should possess in order to enter into a fruitful collision is known as

A)

reaction energy

B)

collision energy

C)

activation energy

D)

threshold energy

View Solution

24)

For a reaction, activation energy \[\left( {{E}_{a}} \right)=0\] and rate constant \[(k)=3.2\times {{10}^{6}}{{s}^{-1}}\] at 300 K. What is the value of the rate constant at 310 K

A)

\[3.2\times {{10}^{-12}}{{s}^{-1}}\]

B)

\[3.2\times {{10}^{6}}{{s}^{-1}}\]

C)

\[6.4\times {{10}^{12}}{{s}^{-1}}\]

D)

\[6.4\times {{10}^{6}}{{s}^{-1}}\]

View Solution

25)

In the Arrhenius plot of ln k Vs\[\frac{1}{T}\], a linear plot is obtained with a slope of \[-2\times {{10}^{4}}K.\] The energy of activation of the reaction (in\[kJ\text{ }mol{{e}^{-1}}\]) is (R value is\[8.3J\text{ }{{K}^{-1}}mo{{l}^{-1}}\])

A)

83

B)

166

C)

249

D)

332

View Solution

26)

The rate of reaction is doubled for every \[10{}^\circ C\] rise in temperature. The increase in reaction rate as a result of temperature rise from \[10{}^\circ C\] to \[100{}^\circ C\] is

A)

112

B)

512

C)

400

D)

614

View Solution

27)

Consider the reaction \[A\to 2B+C,\Delta H=-15\]kcal. The energy of activation of backward reaction is\[20\text{ }kcal\text{ }mo{{l}^{-1}}\]. In presence of catalyst the energy of activation of forward reaction is \[3\text{ }kcal\text{ }mo{{l}^{-1}}\]. At 400 K. the catalyst causes the rate of the reaction to increase by the number of times equal to

A)

\[{{e}^{3.5}}\]

B)

\[{{e}^{2.5}}\]

C)

\[{{e}^{-\,2.5}}\]

D)

\[{{e}^{2.303}}\]

View Solution

28)

A reaction takes place in various steps. The rate constant for first, second, third and fifth steps are \[{{k}_{1}},{{k}_{2}},{{k}_{3}}\] and \[{{k}_{4}}\] respectively The overall rate constant is given by \[k=\frac{{{k}_{2}}}{{{k}_{3}}}{{\left( \frac{{{k}_{1}}}{{{k}_{5}}} \right)}^{1/2}}\]. If activation energy are 40,60,50 and 10 kJ/mol respectively, the overall energy of activation (kJ/ mol) is:

A)

10

B)

20

C)

25

D)

none of these

View Solution

29)

Consider the two hypothetical reactions given below:

I \[a\text{ }A\to \]Products, \[k=x\,mo{{l}^{-1}}\text{ }L\text{ }mi{{n}^{-1}}\]

II \[bB\to \]Products, \[k=y\,mi{{n}^{-1}}\]

The half-lives of both the reactions are the same, equal to 1 hr when molar concentration of the reactant is 1.0 M in each case. If these reactions are started at the same time taking 1M of the reactant in each case, the ratio [A]/[B] after 3 hr will be:

A)

0.5

B)

4

C)

1

D)

2

View Solution

30)

Consider the consecutive reactions: \[A\xrightarrow{k=2\times {{10}^{-5}}{{s}^{-1}}}B\xrightarrow{k=8\times {{10}^{-6}}{{s}^{-1}}}\]\[C\xrightarrow{k=3\times {{10}^{-3}}{{s}^{-1}}}D\] The rate determining step of the reaction is:

A)

\[A\to B\]

B)

\[C\to D\]

C)

\[B\to C\]

D)

\[A\to D\]

View Solution

31)

\[A+2B\to C\], the rate equation for this reaction is given as Rate \[=K\left[ A \right]\left[ B \right].\] If the concentration of A is kept the same but that of B is doubled what will happen to the rate itself?

A)

halved

B)

the same

C)

doubled

D)

quadrupled

View Solution

32)

In the reaction of formation of sulphur trioxide by contact process \[2S{{O}_{2}}+{{O}_{2}}\rightleftharpoons 2S{{O}_{3}}\] the rate of reaction was measured as \[\frac{d[{{O}_{2}}]}{dt}=-2.5\times {{10}^{-4}}mol{{L}^{-1}}{{s}^{-1}}\]. The rate of reaction is terms of \[[S{{O}_{2}}]\] in \[mol\text{ }{{L}^{-1}}{{s}^{-1}}\] will be:

A)

\[-1.25\times {{10}^{-4}}\]

B)

\[-2.50\times {{10}^{-4}}\]

C)

\[-3.75\times {{10}^{-4}}\]

D)

\[-5.00\times {{10}^{-4}}\]

View Solution

33)

For the reaction, \[2{{N}_{2}}{{O}_{5}}\to 4N{{O}_{2}}+{{O}_{2}}\] the rate equation can be expressed in two ways\[-\frac{d[{{N}_{2}}{{O}_{5}}]}{dt}=k[{{N}_{2}}{{O}_{5}}]\] and \[+\frac{d[N{{O}_{2}}]}{dt}=k'[{{N}_{2}}{{O}_{5}}]\] k and k' are related as:

A)

\[k=k'\]

B)

\[2k=k'\]

C)

\[k=2k'\]

D)

\[k=4k'\]

View Solution

34)

The reaction \[2{{N}_{2}}{{O}_{5}}\rightleftharpoons 2{{N}_{2}}{{O}_{4}}+{{O}_{2}}\]

A)

bimolecular and of second order

B)

unimolecular and of first order

C)

bimolecular and of first order

D)

bimolecular and of zero order

View Solution

35)

For the reaction system: \[2NO\left( g \right)+{{O}_{2}}\left( g \right)\to 2N{{O}_{2}}\left( g \right)\] volume is suddenly reduced to half its value by increasing the pressure on it. If the reaction is of first order with respect to \[{{O}_{2}}\] and second order with respect to NO, the rate of reaction will

A)

diminish to one-eighth of its initial value

B)

increase to eight times of its initial value

C)

increase to four times of its initial value

D)

diminish to one-fourth of its initial value

View Solution

36)

Units of rate constant of first and zero order reactions in terms of molarity M unit are respectively

A)

\[se{{c}^{-1}},\text{ }M.se{{c}^{-1}}\]

B)

\[se{{c}^{-1}},\text{ }M\]

C)

\[M.se{{c}^{-1}},\text{ }se{{c}^{-1}}\]

D)

\[M,\text{ }se{{c}^{-1}}\]

View Solution

37)

The plot of concentration of the reactant Vs time for a reaction is a straight line with a negative slope. The reaction follows a rate equation of

A)

zero order

B)

first order

C)

second order

D)

third order

View Solution

38)

The differential rate law for the reaction \[{{H}_{2}}(g)+{{I}_{2}}(g)\to 2HI(g)\] is

A)

\[-\frac{d[{{H}_{2}}]}{dt}=-\frac{d[{{I}_{2}}]}{dt}=-\frac{d[HI]}{dt}\]

B)

\[\frac{d[{{H}_{2}}]}{dt}=\frac{d[{{I}_{2}}]}{dt}=\frac{1}{2}\frac{d[HI]}{dt}\]

C)

\[\frac{1}{2}\frac{d[{{H}_{2}}]}{dt}=\frac{1}{2}\frac{d[{{I}_{2}}]}{dt}=-\frac{d[HI]}{dt}\]

D)

\[-2\frac{d[{{H}_{2}}]}{dt}=-2\frac{d[{{I}_{2}}]}{dt}=\frac{d[HI]}{dt}\]

View Solution

39)

Which of the following will react at the highest rate?

A)

1 mole of A and 1 mole of B in a 1 -L vessel

B)

2 mole of A and 2 mole of B in a 2-L vessel

C)

3 mole of A and 3 mole of B in a 3-L vessel

D)

All would react at the same rate

View Solution

40)

In the reaction,\[A+2B\xrightarrow{{}}6C+2D\], If the initial rate \[-\frac{d[A]}{dt}\] at t = 0 is \[2.6\times {{10}^{-2}}M\text{ }se{{c}^{-1}}\] what will be the value of \[\frac{d[B]}{dt}\] at\[t=0\]?

A)

\[8.5\times {{10}^{-2}}M\text{ }se{{c}^{-1}}\]

B)

\[2.5\times {{10}^{-2}}M\text{ }se{{c}^{-1}}\]

C)

\[5.2\times {{10}^{-2}}M\text{ }se{{c}^{-1}}\]

D)

\[7.5\times {{10}^{-2}}M\text{ }se{{c}^{-1}}\]

View Solution

41)

The reaction \[L\xrightarrow{{}}M\] is started with 10.0 g of L. After 30 and 90 minutes 5.0 g and 1.25 g of L respectively are left. The order of the reaction is

A)

0

B)

1

C)

2

D)

3

View Solution

42)

A first order reaction is half-completed in 45 minutes. How long does it need for 99.9% of the reaction to be completed?

A)

20 hours

B)

10 hours

C)

\[7\frac{1}{2}\] hours

D)

5 hours

View Solution

43)

A reaction which is of first order w.r.t. reactant A, has a rate constant 6 \[{{\min }^{-1}}\]. If we start with \[\left[ A \right]=0.5\text{ }mol\text{ }{{L}^{-1}}\], when would [A] reach the value of \[0.05\text{ }mol\,{{L}^{-1}}\]

A)

0.384 min

B)

0.15 min

C)

3 min

D)

3.84 min

View Solution

44)

The time taken for 90% of a first order reaction to complete is approximately

A)

1.1 times that of half-life

B)

2.2 times that of half-life

C)

3.3 times that of half-life

D)

4.4 times that of half-life

View Solution

45)

The rate constant of a reaction is\[0.0693\text{ }mi{{n}^{-1}}\]. Starting with 10 mol, the rate of the reaction after 10 minis

A)

\[0.0693\text{ }mol\text{ }mi{{n}^{-1}}\]

B)

\[0.0693\times 2\text{ }mol\text{ }mi{{n}^{-1}}\]

C)

\[0.0693\times 5\text{ }mol\text{ }mi{{n}^{-1}}\]

D)

\[0.0693\times {{\left( 5 \right)}^{2}}mol\text{ }mi{{n}^{-1}}\]

View Solution

46)

The plot that represents the zero order reaction is:

A)

B)

C)

D)

View Solution

47)

Which of the following reactions is not of the first order?

A)

Inversion of sucrose in the presence of acid

B)

Acid-catalyzed hydrolysis of ethyl acetate

C)

Hydrolysis of tertiary butyl halide using alkali

D)

Oxidation of \[{{I}^{-}}\]ion by \[{{S}_{2}}O_{8}^{2-}\] ion

View Solution

48)

A first order reaction is 50% completed in 20 minutes at \[27{}^\circ C\] and in 5 minutes at\[47{}^\circ C\]. The energy of activation of the reaction is:

A)

43.85 kJ/mol

B)

55.14 kJ/mol

C)

11.97 kJ/mol

D)

6.65 kJ/mol

View Solution

49)

For the first order reaction \[A\xrightarrow{{}}B+C\] is carried out at\[27{}^\circ C\]. If \[3.8\times {{10}^{-16}}\] % of the reactant molecules exists in the activated state, the \[{{E}_{4}}\](activation energy) of the reaction is:

A)

12 kJ/mol

B)

831.4 kJ/mol

C)

100 kJ/mol

D)

88.57 kJ/mol

View Solution

50)

A catalyst lowers the activation energy of a certain reaction from 83.314 to \[75\text{ }kJ\text{ }mo{{l}^{-1}}\] at 500 K. What will be the rate of reaction as compared to uncatalysed reaction? Assume other things being equal.

A)

Double

B)

28 times

C)

7.38 times

D)

\[7.38\times {{10}^{3}}\]times

View Solution

51)

Rate of a reaction can be expressed by Arrhenius equation as: \[k=A{{e}^{-{{E}_{a}}}}^{/RT}\] In this equation, \[{{E}_{a}}\] represents

A)

the total energy of the reacting molecules at a temperature, T

B)

the fraction of molecules with energy greater than the activation energy of the reaction

C)

the energy below which all the colliding molecules will react

D)

the energy below which colliding molecules will not react

View Solution

52)

The reason for almost doubling the rate of reaction on increasing the temperature of the reaction system by \[10{}^\circ C\] is

A)

The value of threshold energy increases

B)

Collision frequency increases

C)

The fraction of the molecule having energy equal to threshold energy or more increases

D)

Activation energy decreases

View Solution

53)

In Arrhenius plot, intercept is equal to

A)

\[\frac{-{{E}_{a}}}{R}\]

B)

\[\ell nA\]

C)

\[\ell n\,K\]

D)

\[lo{{g}_{10}}A\]

View Solution

54)

A reaction rate constant is given by \[k=1.2\times {{10}^{14}}{{e}^{-25000/RT}}se{{c}^{-1}}\]. It means

A)

log k versus log T will give a straight line with a slope as \[-25000\]

B)

log k versus T will give a straight line with slope as 25000

C)

log k versus 1/T will give a straight line with slope as \[-25000/R\]

D)

log k versus 1/T will give a straight line

View Solution

55)

The velocity of a reaction is doubled for every \[10{}^\circ C\] rise in temp. If the temp. is raised to \[50{}^\circ C\]from \[0{}^\circ C\] the reaction velocity increases by about

A)

12 times

B)

16 times

C)

32 times

D)

50 times

View Solution

56)

Which of the following statements is incorrect?

A)

Activation energy for the forward reaction is equals to activation energy for the reverse reaction

B)

For a reversible reaction, an increase in temperature increases the reaction rate for both the forward and the backward reaction

C)

The larger the initial reactant concentration for a second order reaction, the shorter is its half-life.

D)

When \[\Delta t\] is infinitesimally small, the average rate equals the instantaneous rate

View Solution

57)

Consider the following statements:

I. Increase in concentration of reactant increases the rate of a zero order reaction.

II. Rate constant k is equal to collision frequency A if \[{{E}_{a}}=0.\]

III. Rate constant k is equal to collision frequency A if \[{{E}_{a}}=\infty .\]

IV. In k Vs T is a straight line.

V. In k Vs 1/T is a straight line.

Correct statements are

A)

I and IV

B)

II and V

C)

III and IV

D)

II and III

View Solution

58)

The time required for 10% completion of a first order reaction at 298 K is equal to that required for its 25% completion at 308 K, If the pre-exponential factor for the reaction is \[3.56\times {{10}^{9}}{{s}^{-1}}\] the rate constant at 318 K is:

A)

\[18.39\text{ }kcal\text{ }mo{{l}^{-1}}\]

B)

\[20\,kcal\,mo{{l}^{-1}}\]

C)

\[16\,kcal\,mo{{l}^{-1}}\]

D)

\[21.5\,kcal\,mo{{l}^{-1}}\]

View Solution

59)

For the reaction, \[3A+2B\to C+D\], the differential rate law can be written as:

A)

\[\frac{1}{3}\frac{d[A]}{dt}=\frac{d[C]}{dt}=k{{[A]}^{n}}{{[B]}^{m}}\]

B)

\[-\frac{d[A]}{dt}=\frac{d[C]}{dt}=k{{[A]}^{n}}{{[B]}^{m}}\]

C)

\[+\frac{1}{3}\frac{d[A]}{dt}=-\frac{d[C]}{dt}=k{{[A]}^{n}}{{[B]}^{m}}\]

D)

\[-\frac{1}{3}\frac{d[A]}{dt}=\frac{d[C]}{dt}=k{{[A]}^{n}}{{[B]}^{m}}\]

View Solution

60)

The instantaneous rate of disappearance of \[MnO_{4}^{-}\] ion in the following reaction is

\[4.56\times {{10}^{-3}}M{{s}^{-1}}2MnO_{4}^{-}+10{{I}^{-}}+16{{H}^{+}}\to \] \[2M{{n}^{2+}}+5{{I}_{2}}+8{{H}_{2}}O\]

The rate of appearance \[{{I}_{2}}\] is:

A)

\[4.56\times {{10}^{-4}}M{{s}^{-1}}\]

B)

\[1.14\times {{10}^{-2}}M{{s}^{-1}}\]

C)

\[1.14\times {{10}^{-3}}M{{s}^{-1}}\]

D)

\[5.7\times {{10}^{-3}}M{{s}^{-1}}\]

View Solution

61)

The rate constant of a zero order reaction is\[2.0\times {{10}^{-2}}mol\,{{L}^{-1}}{{s}^{-1}}\]. If the concentration of the reactant after 25 seconds is 0.5 M. What is the initial concentration?

A)

0.5 M

B)

1.25 M

C)

12.5 M

D)

\[1.0\,M\]

View Solution

62)

The reaction \[A\to B\] follows first order kinetics. The time taken for 0.8 mole of A to produce 0.6 mole of B is 1 hour. What is the time taken for conversion of 0.9 mole of A to produce 0.675 mole of B?

A)

2 hours

B)

1 hour

C)

0.5 hour

D)

0.25 hour

View Solution

63)

The rate of a first order reaction is \[1.5\times {{10}^{-2}}mol\text{ }{{L}^{-1}}{{\min }^{-1}}\] at 0.5 M concentration of the reactant. The half-life of the reaction is

A)

0.383 min

B)

23.1 min

C)

8.73 min

D)

7.53 min

View Solution

64)

For a first order reaction \[A\to B\] the reaction rate at reactant concentration of 0.01 M is found to be\[2.0\times {{10}^{-5}}mol\text{ }{{L}^{-1}}\text{ }{{s}^{-1}}\]. The half-life period of the reaction is

A)

30 s

B)

220 s

C)

300 s

D)

347 s

View Solution

65)

A reaction proceeds by first order, 75% of this reaction was completed in 32 min. The time required for 50% completion is

A)

8 min

B)

16 min

C)

20 min

D)

24 min

View Solution

66)

Consider the reaction: \[{{N}_{2}}(g)+3{{H}_{2}}(g)\to 2N{{H}_{3}}(g)\] The equality relationship between \[\frac{d[N{{H}_{3}}]}{dt}\] and \[-\frac{d[{{H}_{2}}]}{dt}\] is

A)

\[+\frac{d[N{{H}_{3}}]}{dt}=-\frac{2}{3}\frac{d[{{H}_{2}}]}{dt}\]

B)

\[+\frac{d[N{{H}_{3}}]}{dt}=-\frac{3}{2}\frac{d[{{H}_{2}}]}{dt}\]

C)

\[\frac{d[N{{H}_{3}}]}{dt}=-\frac{d[{{H}_{2}}]}{dt}\]

D)

\[\frac{d[N{{H}_{3}}]}{dt}=-\frac{1}{3}\frac{d[{{H}_{2}}]}{dt}\]

View Solution

67)

The rate of a reaction increases four-fold when the concentration of reactant is increased 16 times. If the rate of reaction is \[4\times {{10}^{-6}}mol\text{ }{{L}^{-1}}\text{ }{{s}^{-1}}\]when the concentration of the reactant is\[4\times {{10}^{-4}}mol\text{ }{{L}^{-1}}\]. The rate constant of the reaction will be

A)

\[2\times {{10}^{-4}}mo{{l}^{1/2}}{{L}^{-1/2}}{{s}^{-1}}\]

B)

\[1\times {{10}^{-2}}{{s}^{-1}}\]

C)

\[2\times {{10}^{-4}}mo{{l}^{-1/2}}{{L}^{1/2}}{{s}^{-1}}\]

D)

\[25\text{ }mo{{l}^{-1}}L\text{ }mi{{n}^{-1}}\]

View Solution

68)

In the reaction\[A\to B+C\], rate constant is\[0.001\text{ }M{{s}^{-1}}\]. If we start with 1 M of A then cone. of A and B after 10 minuter are respectively.

A)

0.5 M, 0.5 M

B)

0.6 M, 0.4 M

C)

0.4 M, 0.6 M

D)

0.6 M 0.5 M

View Solution

69)

The half-life for the virus inactivation if in the beginning 1.5% of the virus is inactivated per minute is (Given: The reaction is of first order)

A)

76 min

B)

66 min

C)

56 min

D)

46 min

View Solution

70)

The reaction of \[{{A}_{2}}\] and \[{{B}_{2}}\] follows the equation \[{{A}_{2}}(g)+{{B}_{2}}(g)\to 2AB(g)\] The following data were observed

\[{{[{{A}_{2}}]}_{0}}\]	\[{{[{{B}_{2}}]}_{0}}\]	Initial rate of appearance of \[AB(g)\,(in\,M{{s}^{-1}})\]
0.10	0.10	\[2.5\times {{10}^{-4}}\]
0.20	0.10	\[5\times {{10}^{-4}}\]
0.20	0.20	\[10\times {{10}^{-4}}\]

The value of rate constant for the above reaction is:

A)

\[2.5\times {{10}^{-4}}\]

B)

\[2.5\times {{10}^{-2}}\]

C)

\[1.25\times {{10}^{-2}}\]

D)

None of these

View Solution

71)

In the presence of an acid, the initial concentration of cane sugar was reduced from 0.20 to 0.10 M in 5 hours and from 0.2 to 0.05 M in 10 hours. The reaction is of;

A)

Zero order

B)

First order

C)

Second order

D)

Third order

View Solution

72)

The activation energies of the forward and backward reactions in the case of a chemical reaction are 30.5 and 45.4 kJ/mol respectively. The reaction is:

A)

exothermic

B)

endothermic

C)

neither exothermic nor endothermic

D)

independent of temperature

View Solution

73)

A homogeneous catalytic reaction takes place through the three alternative plots A, B and C shown in the given figure. Which one of the following indicates the relative ease with which the reaction can take place?

A)

A>B>C

B)

C>B>A

C)

A>C>B

D)

A=B=C

View Solution

74)

A catalyst is a substance which:

A)

is always in the same phase as in the reaction

B)

alters the equilibrium in a reaction

C)

does not participate in the reaction but alters the rate of reaction

D)

participates in the reaction and provides an easier pathway for the same

View Solution

75)

For an exothermic reaction, the energy of activation of the reactants is

A)

equal to the energy of activation of products

B)

less than the energy of activation of products

C)

greater than the energy of activation of products

D)

sometimes greater and sometimes less than that of the products

View Solution

76)

When a biochemical reaction is carried out in laboratory in the absence of enzyme then rate of reaction obtained is \[{{10}^{-6}}\] times, then activation energy of reaction in the presence of enzyme is

A)

\[\frac{6}{RT}\]

B)

different from \[{{E}_{a}}\] obtained in laboratory,

C)

P is required

D)

can't say anything

View Solution

77)

A chemical reaction was carried out at 300 K and 280 K. The rate constants were found to be \[{{k}_{1}}\] and \[{{k}_{2}}\] respectively, then

A)

\[{{k}_{2}}=4{{k}_{1}}\]

B)

\[{{k}_{2}}=2{{k}_{1}}\]

C)

\[{{k}_{2}}=0.25\,{{k}_{1}}\]

D)

\[{{k}_{2}}=0.5{{k}_{1}}\]

View Solution

78)

In a reaction at \[27{}^\circ C,{{10}^{-3}}\]% reactant molecules manage to cross over the barrier of transition state. The energy of these molecules in excess of the average value will be \[(R=2cal\text{ }{{K}^{-1}}\text{ }mo{{l}^{-1}})\]:

A)

\[6.91\text{ kc}al\text{ }mo{{l}^{-1}}\]

B)

\[3.00\text{ kc}al\text{ }mo{{l}^{-1}}\]

C)

\[4.15\,kcal\,mo{{l}^{-1}}\]

D)

\[5.10kcal\,mo{{l}^{-1}}\]

View Solution

79)

The activation energy for a simple chemical reaction \[A\to B\] is \[{{E}_{a}}\] in forward direction. The activation energy for reverse reaction

A)

is always double of \[{{E}_{a}}\]

B)

is negative of \[{{E}_{a}}\]

C)

is always less than \[{{E}_{a}}\]

D)

can be less than or more than \[{{E}_{a}}\]

View Solution

80)

The slope in Arrhenius plot, is equal to:

A)

\[-\frac{{{E}_{a}}}{2.303R}\]

B)

\[\frac{{{E}_{a}}}{R}\]

C)

\[-\frac{R}{2.303{{E}_{a}}}\]

D)

None of these

View Solution

81)

A radioactive isotope having a half - life period of 3 days was received after 12 days. If 3g of the isotope is left in the container, what would be the initial mass of the isotope?

A)

12g

B)

36g

C)

48g

D)

24g

View Solution

82)

In a chemical reaction A is converted into B. The rates of reaction, starting with initial concentrations of A as \[2\times {{10}^{-3}}M\] and \[1\times {{10}^{-3}}M,\] are equal to \[2.40\times {{10}^{-4}}M{{s}^{-1}}\] and \[0.60\times {{10}^{-4}}M{{s}^{-1}}\] respectively. The order of reaction with respect to reactant A will be

A)

0

B)

1.5

C)

1

D)

2

View Solution

83)

For a reaction \[A\to \] Products, a plot of log \[{{t}_{1/2}}\]versus \[\log {{a}_{0}}\] is shown in the figure. If the initial concentration of A is represented by \[{{a}_{0}}\], the order of the reaction is

A)

one

B)

zero

C)

two

D)

three

View Solution

84)

The rate constant of a reaction with a virus is \[3.3\times {{10}^{-4}}{{s}^{-1}}\]. Time required for the virus to become 75% inactivated is

A)

35 min

B)

70 min

C)

105 min

D)

17.5 min

View Solution

85)

A Geigger Muller counter is used to study the radioactive process. In the absence of radioactive substance A, it counts 3 disintegration per second (dps). At the start in the presence of A, it records 23 dps; and after 10 min 13 dps,

(i) What does it count after 20 min

(ii) What is the half life of A?

A)

8 dps, 10 min

B)

5 dps, 10 min

C)

5 dps, 20 min

D)

5 dps, 5 min

View Solution

86)

The half life period for catalytic decomposition of \[A{{B}_{3}}\] at 50 mm Hg is 4 hrs and at 100 mm Hg it is 2 hrs. The order of reaction is

A)

1

B)

3

C)

2

D)

0

View Solution

87)

The rate equation for a reaction, \[{{N}_{2}}O\xrightarrow{{}}{{N}_{2}}+1/2{{O}_{2}}\] is Rate \[=k{{[{{N}_{2}}O]}^{0}}=k.\] If the initial concentration of the reactant is a mol\[Li{{t}^{-1}}\], the half-life period of the reaction is

A)

\[{{t}_{\frac{1}{2}}}=\frac{a}{2k}\]

B)

\[-{{t}_{\frac{1}{2}}}=ka\]

C)

\[{{t}_{\frac{1}{2}}}=\frac{a}{k}\]

D)

\[{{t}_{\frac{1}{2}}}=\frac{k}{a}\]

View Solution

88)

The rate constant for a first order reaction whose half life is 480 sec, is:

A)

\[1.44\times {{10}^{-3}}se{{c}^{-1}}\]

B)

\[1.44\times se{{c}^{-1}}\]

C)

\[0.72\times {{10}^{-3}}se{{c}^{-1}}\]

D)

\[2.88\times {{10}^{-3}}se{{c}^{-1}}\]

View Solution

89)

The hypothetical reaction \[{{A}_{2}}+{{B}_{2}}\xrightarrow{{}}2AB\]; follows the following mechanism \[{{A}_{2}}\xrightarrow{Fast}A+A,\] \[A+{{B}_{2}}\xrightarrow{slow}AB+B,A+B\xrightarrow{Fast}AB\] The order of the overall reaction is

A)

0

B)

1

C)

2

D)

3/2

View Solution

90)

If half-life of a substance is 5 yrs, then the total amount of substance left after 15 years, when initial amount is 64 grams is

A)

16g

B)

2g

C)

32g

D)

8g

View Solution

91)

In a reversible reaction the energy of activation of the forward reaction is 50 kcal. The energy of activation for the reverse reaction will be

A)

< 50 kcal

B)

either greater than or less than 50 kcal

C)

50 kcal

D)

> 50 kcal

View Solution

92)

Activation energy of a chemical reaction can be determined by

A)

evaluating rate constant at standard temperature

B)

evaluating velocities of reaction at two different temperatures

C)

evaluating rate constants at two different temperatures

D)

changing concentration of reactants

View Solution

93)

For the exothermic reaction \[A+B\to C+D,\text{ }\Delta H\]is the heat of reaction and \[{{E}_{a}}\]is the energy of activation. The energy of activation for the formation of A + B will be

A)

\[{{E}_{a}}\]

B)

\[\Delta H\]

C)

\[{{E}_{a}}+\Delta H\]

D)

\[\Delta H-{{E}_{a}}\]

View Solution

94)

A reaction having equal energies of activation for forward and reverse reaction has:

A)

\[\Delta G=0\]

B)

\[\Delta H=0\]

C)

\[\Delta H=\Delta G=\Delta S=0\]

D)

\[\Delta S=0\]

View Solution

95)

The rate coefficient (K) for a particular reactions is \[1.3\times {{10}^{-4}}{{M}^{-1}}{{s}^{-1}}\] at\[100{}^\circ C\], and \[1.3\times {{10}^{-3}}{{M}^{-1}}{{s}^{-1}}\] at\[150{}^\circ C\]. What is the energy of activation \[\left( {{E}_{a}} \right)\] (in kJ) for this reaction? (R = molar gas constant\[=8.314\text{ }J{{K}^{-1}}mo{{l}^{-1}}\])

A)

16

B)

60

C)

99

D)

132

View Solution

96)

The reaction \[X\to Y\] is an exothermic reaction. Activation energy of the reaction for X into Y is\[150\,kJ\,mo{{l}^{-1}}\]. Enthalpy of reaction is\[135\text{ }k\,J\,mo{{l}^{-1}}\]. The activation energy for the reverse reaction, \[Y\to X\] will be:

A)

\[280\,kJ\,mo{{l}^{-1}}\]

B)

\[285\text{ }kJmo{{l}^{-1}}\]

C)

\[270\text{ }kJ\,mo{{l}^{-1}}\]

D)

\[15\,kJ\,mo{{l}^{-1}}\]

View Solution

97)

The activation energy for a reaction which doubles the rate when the temperature is raised from 298 K to 308 K is

A)

\[59.2\text{ }kJ\,mo{{l}^{-1}}\]

B)

\[39.2\text{ kJ }mo{{l}^{-1}}\]

C)

\[52.9\,kJ\,mo{{l}^{-1}}\]

D)

\[29.5\,kJ\,mo{{l}^{-1}}\]

View Solution

98)

\[{{t}_{1/4}}\] can be taken as the time taken for the concentration of a reactant to drop to \[\frac{3}{4}\] of its initial value. If the rate constant for a first order reaction is k, the \[{{t}_{1/4}}\] can be written as

A)

\[0.75/k\]

B)

\[0.69/k\]

C)

\[0.29/k\]

D)

\[0.10/k\]

View Solution

99)

\[A\to B,\Delta H=10kJ\,mo{{l}^{-1}},{{E}_{a(f)}}=50kJ\,mo{{l}^{-1}}\], then \[{{E}_{a}}\] of \[B\to A\] will be

A)

\[40kJ\,mo{{l}^{-1}}\]

B)

\[50kJ\,mo{{l}^{-1}}\]

C)

\[-50kJ\,mo{{l}^{-1}}\]

D)

\[60kJ\,mo{{l}^{-1}}\]

View Solution

100)

For a certain reaction, rate\[=k\times {{\left[ {{H}^{+}} \right]}^{n}}\]. If pH of reaction changes from two to one, the rate becomes 100 times of its value at pH = 2, the order of reaction is-

A)

1

B)

2

C)

0

D)

3

View Solution

NEET Chemistry Chemical Kinetics / रासायनिक बलगतिकी Question Bank

done Self Evaluation Test - Chemical Kinetics Total Questions - 100

Study Package

Self Evaluation Test - Chemical Kinetics

Self Evaluation Test - Chemical Kinetics Total Questions - 100