Chemical Kinetics = B5P

1. For the reaction $2X + Y \rightarrow P$; Rate of reaction is ${d[P] \over dt} = k[X]$.
4 Moles of 'X' are mixed with 2 moles of Y to make a 1.0 L solution. At 69.3 minutes, 2 moles of 'X' are consumed.
Read the following statements about the reaction and select the correct ones: (Given $ln2 = 0.693$)

(a)	Time required to consume 3 moles of X is $2 \times 69.3 $ minutes
(b)	Value of $k = { ln2 \over 2 \times 0.693 } min^{-1}$
(c)	$-\frac{d x}{d t}=2 \times 10^{-2} \frac{\mathrm{~m}}{\mathrm{~min}}~ at ~t=69.3 \mathrm{~min}$
(d)	$\frac{d y}{d t}=5 \times 10^{-3} \frac{\mathrm{~m}}{\mathrm{min}}~ at~t=138.6 \mathrm{~min}$

Choose the correct options:
1. (a), (b), (c) and (d)
2. (a), (b) and (d)
3. (a), (c) and (d)
4. None of the above

2. Given below are two graphs:

Graph I:
Graph II:

In the light of the above two graphs, choose the correct answer from the options given below :

1.	Both graph I and graph II are not correct.
2.	Graph I is not correct but graph II is correct.
3.	Both graph I and graph II are correct.
4.	Graph I is correct, but graph II is not correct.

3. Which of the following statements is/are correct?

(i)	A catalyst lowers the activation energy of a reaction.
(ii)	A catalyst allows the same rate of reaction to be achieved at a lower temperature.
(iii)	A catalyst mixes with the reactants and increases the overall concentration of reactants in the rate equation.

1. i only
2. i and ii only
3. ii and iii only
4. i, ii, and iii

4. Consider the given reaction:
$A(g) \xrightarrow{k=0.1 M \min ^{-1}} 2 B(\mathrm{~g}) $
If the initial concentration of A is 0.5 M, which of the following graphs correctly represents the concentration of B over time?

1.		2.
3.		4.

5. The activation energy of one of the reactions in a biochemical process is $\mathrm{532611~ J~ mol^{–1} .}$ When the temperature falls from $\mathrm{310~ K}$ to $\mathrm{300~ K,}$ the change observed in the rate constant is $\mathrm{k_{300} = x × 10^{–3} k_{310}.}$
The value of $\mathrm{x}$ is:
[Given: ln$\mathrm{10 = 2.3, R = 8.3 ~JK^{–1} mol^{–1}}$]

1.	1	2.	5
3.	2	4.	8

6. Two first-order reactions have half-lives in the ratio. Calculate the ratio of
the time intervals $t_1: t_2$where the time $t_1$ and $t_2$ are the time periods
for $\left(\frac{1}{4}\right)^{\mathrm{th}}$ and $\left(\frac{3}{4}\right)^{\mathrm{th}}$ completion of the reaction, respectively.
1. $1: 0.301$
2. $0.125: 0.602$
3. $1: 602$
4. None of the above

7. What is the rate constant for a reaction if the time taken by the first-order decomposition of $\text{SO}_2\text{Cl}_2$ to decompose to 40% is 560 seconds?
[Given: log 2.5 = 0.3979]

1.	$2.726 \times 10^{-5} \mathrm{~min}^{-1}$	2.	$2.276 \times 10^{-5} \mathrm{~min}^{-1}$
3.	$2.216 \times 10^{-5} \mathrm{~min}^{-1}$	4.	None of the above

8. For a reaction $2 A+B \longrightarrow P, $ when concentration of B alone is doubled $t_{1 / 2}$ does not change and when concentration of both A and B is doubled, rate increases by a factor of 4. The unit of rate constant is:

1.	$\mathrm{s}^{-1}$	2.	$\mathrm{L} \mathrm{mol}^{-1} \mathrm{~s}^{-1}$
3.	$\mathrm{mol} \mathrm{L}^{-1} \mathrm{~s}^{-1}$	4.	$\mathrm{L}^2 \mathrm{~mol}^{-2} \mathrm{~s}^{-1}$

9. Arrhenius equation may be represented as:

(a)	$\ln\dfrac{A}{k}=\dfrac{E_a}{R T}$
(b)	$\dfrac{d \ln k}{d T}=\dfrac{E_a}{R T^2}$
(c)	$\log A=\log k+\dfrac{E_a}{2.303 R T}$
(d)	$\log \left(-\dfrac{E_a}{R T}\right)=\dfrac{k}{A}$

Choose the correct option:
1. a, b and c
2. b, c and d
3. c and d
4. None of the above

10. Which of the following statements is true regarding the nature of reaction order and reaction mechanisms?

1.	A second-order reaction is always a multistep reaction.
2.	A zero-order reaction is a multistep reaction.
3.	A first-order reaction is always a single-step reaction.
4.	A zero-order reaction is a single-step reaction.

11. Which of the following statements is always true about the kinetics of a chemical reaction?

1.	The rate law includes all reactants in the balanced overall equation.
2.	The overall order equals the sum of the reactant coefficients in the overall reaction.
3.	The overall order equals the sum of the reactant coefficients in the slow step of the reaction.
4.	The structure of the catalyst remains unchanged throughout the reaction progress.

12. The correct rate law for the given balanced reaction is :
$4A\,+\,2B$ → $C \,+\,3D$
1. Rate = k[A]⁴[B]²
2. Rate = k[A]²[B]
3. Rate = k[C][D]³/[A]⁴[B]²
4. Cannot be determined from the information given.

13. Given below are two statements:

Assertion (A):	A reaction can have zero activation energy.
Reason (R):	The minimum amount of energy required by reactant molecules so that their energy becomes equal to threshold value, is called activation energy.

1.	(A) is False but (R) is True.
2.	Both (A) and (R) are True and (R) is the correct explanation of (A)
3.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
4.	(A) is True but (R) is False.

14.

Thermal decomposition of $Cl_2O_7$ at 400 K in the gaseous phase to $Cl_2$ and $O_2$ is a first order reaction with rate constant $6.932 \times 10^{-3} s^{-1}$. The time (in minutes) required for 90% decomposition of $Cl_2O_7$ at 400 K is:

1.	5.54	2.	16.61
3.	33.32	4.	332.2

15. For the reaction A + B → C, experiments were performed in the presence of a large amount of B to measure the initial reaction rate (V_f) as a function of the initial concentration of A ([A]₀). The data from the experiments are plotted as shown below. The order of the reaction with respect to A is:

1. 1
2. 3
3. 2/3
4. 3/2

16. Read the following statements:

(i)	The thermal decomposition of HI on a gold surface follows a zero-order reaction.
(ii)	Instantaneous rate = $\operatorname{limit}_{t \rightarrow 0} \frac{\Delta C}{\Delta t}$
(iii)	The rate of 1^st order reaction is proportional to the first power of the concentration of the reactant.
(iv)	Radioactive reaction follows 1^storder kinetics.

The correct statements are:
1. (i), (ii)
2. (i), (iii), (iv)
3. (ii), (iii), (iv)
4. (i), (ii), (iii), (iv)

17. Consider the given two statements:

Assertion(A):	The active complex is an intermediate product.
Reason(R):	The active complex is unstable because of high energy.

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	(A) is False but (R) is True.

18. Given below are two statements:
Assertion(A): The catalyst can increase the rate constant to a large extent.
Reason(R): By using a suitable catalyst, we can increase the rate of reaction.
1. Both A and R are correct and R is the correct explanation of A.
2. Both A and R are correct but R is not the correct explanation of A.
3. A is true and R is false
4. A is false and R is true

19. For an exothermic reaction, the value of $\Delta H$ will be
1. More than $E_a$
2. Less than $E_a$
3. Equal to $E_a$
4. All of the above

20. Consider the following first order reaction:
A(g) → B(g) + C(g) + D(g)
The initial pressure is P and the pressure at a time 't' is P_t (P_t > P). The value of rate constant (K) will be
1. $\frac{2.303}{t}log\frac{P}{P_t}$
2. $\frac{2.303}{t}log\frac{P}{2P-P_t}$
3. $\frac{2.303}{t}log\frac{2P}{3P-P_t}$
4. $\frac{2.303}{t}log\frac{2P}{2P-P_t}$

21. The value of the rate constant depends on:
(a) Concentration
(b) Catalyst
(c) Temperature
1. (a) only
2. (b), (c) only
3. (a), (b) only
4. (c) only

22. Consider the following reversible reaction:

(where K₁ is the rate constant for the forward reaction and K₂ is the rate constant for the backward reaction)
The rate law for the appearance of NH₃ is:
$1.~K_{2}\left[NH_{3}\right]^2 -K_1\left[N_{2}\right][H_2]^{3}\\ 2.~2\mathrm{{~K}_{1}\left[{~N}_{2}\right]\left[{H}_{2}\right]^{3}-2 {~K}_{2}\left[{NH}_{3}\right]^{2}}\\ 3.~2 \mathrm{{~K}_{2}\left[{NH}_{3}\right]^{2}-2 {~K}_{1}\left[{~N}_{2}\right]\left[{H}_{2}\right]^{3}}\\ 4.~\mathrm{{K}_{1}\left[{~N}_{2}\right]\left[{H}_{2}\right]^{3}-{K}_{2}\left[{NH}_{3}\right]^{2}}$

23. Given below are two statements:

Assertion (A):	Inversion of cane sugar is a first-order reaction.
Reason (R):	Inversion of cane sugar is a pseudo-unimolecular reaction.

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True, but (R) is False.
4.	Both (A) and (R) are False.

24. The activation energy for the reaction 2HI_(g) → H₂ + I_2(g) is 209.5 kJ mol⁻¹ at 581K. The fraction of molecules of reactants having energy equal to or greater than activation energy is-
1. 2.67 × 10⁻¹⁹
2. 3.57 × 10⁻¹⁸
3. 4.67 × 10⁻¹⁷
4. 1.47 × 10⁻¹⁹

25. What is the pre-exponential factor for a reaction at 500 K with a rate constant of 0.02 s⁻¹ and an activation energy of 18.230 kJ?
1. 1.61
2. 1.41
3. 1.81
4. 1.21

26.

Consider the reaction, 2A + B → Products.
When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:
1. L mol^–1 s^–1
2. no unit
3. mol L^–1s^–1
4. s^–1

27.

The rate of a reaction is decreased by 3.555 times when the temperature was changed from 40°C to 30°C. The activation energy (in kJ ${mol}^{- 1}$ ) of the reaction is:
(Take R=8.314 J ${mol}^{- 1} K^{- 1}$ and In 3.555=1.268)
1. 100 kJ/mol
2. 120 kJ/mol
3. 95 kJ/mol
4. 108 kJ/mol

28.

₉₂U²³⁵, nucleus absorb a neutron and disintegrate in ₅₄Xe¹³⁹, ₃₈Sr⁹⁴ and x . The product x is:
1. 3 - neutrons
2. 2 - neutrons
3. α - particle
4. β - particle

29.

If the concentration of a solution is changed from 0.2 to 0.4, then what will be rate and rate constant. The reaction is of first order and rate constant is $K = 1 \times 10^{- 6}$ :
1. $2 \times 10^{- 7}$ $;$ $1 \times 10^{- 6}$
2. $1 \times 10^{- 7}$ $;$ $1 \times 10^{6}$
3. $4 \times 10^{- 7}$ $;$ $1 \times 10^{- 6}$
4. $2 \times 10^{- 3}$ $;$ $1 \times 10^{- 3}$

30.

The graphs that represent a zero-order reaction are:

(a)		(b)
(c)		(d)

1.	a and b	2.	b and c
3.	c and d	4.	a and d

31.

The correct statements among following about Maxwell, Boltzmann distribution of energy is -

(a)	The fraction of molecules with the most probable kinetic energy decreases at higher temperatures
(b)	The fraction of molecules with the most probable kinetic energy increases at higher temperatures
(c)	Most probable kinetic energy increases at higher temperatures
(d)	Most probable kinetic energy decreases at higher temperatures

1. (a, b)
2. (b, c)
3. (c, d)
4. (a, c)

32.

The value of the rate constant of a pseudo-first-order reaction:

1.	Depends on the concentration of reactants present in a small amount.
2.	Depends on the concentration of reactants present in excess.
3.	Is independent of the concentration of reactants.
4.	Depends only on temperature.

33.

An incorrect statement about the collision theory of chemical reaction is:

1.	It considers reacting molecules or atoms to be hard spheres and ignores their structural features.
2.	The number of effective collisions determines the rate of reaction.
3.	The collision of atoms or molecules possessing sufficient threshold energy results in product formation.
4.	Molecules should collide in the proper orientation for the collision to be effective with sufficient threshold energy and proper orientation.

34.

Consider the graph given in the figure. Which of the following options does not show an instantaneous rate of reaction in the 40s?

1. ${V_5 -V_2 \over 50-30}$
2. ${V_4 -V_2 \over 50-30}$
3. ${V_3 -V_2 \over 40-30}$
4. ${V_3 -V_1 \over 40-20}$

35.

A graph of volume of hydrogen released vs time for the reaction between zinc and dil. HCl is given in the graph below.

The correct statement among the following based on the graph given above is:
$1 . Average rate upto 40 s is \frac{V_{3} - V_{2}}{40} 2 . Average rate upto 40 s is \frac{V_{3} - V_{2}}{40 - 30} 3 . Average rate upto 40 s is \frac{V_{3}}{40} 4 . Average rate upto 40 s is \frac{V_{3} - V_{1}}{40 - 20}$

36.

For a reaction A → Product, with k = 2.0 × 10^–2s^–1, if the initial concentration of A is 1.0 mol L^–1, the concentration of A after 100 seconds would be :

1.	0.23 mol L^–1	2.	0.18 mol L^–1
3.	0.11 mol L^–1	4.	0.13 mol L^–1

37.

The rate constant for the decomposition of hydrocarbons is 2.418 × 10^–5s^–1 at 546 K. If the energy of activation is 179.9 kJ/mol, the value of the pre-exponential factor will be:
1. $4.0$ $\times$ $10^{12}$ $s^{- 1}$
2. $7.8$ $\times$ $10^{- 13}$ $s^{- 1}$
3. $3.8$ $\times$ $10^{- 12}$ $s^{- 1}$
4. $4.7$ $\times$ $10^{12}$ $s^{- 1}$

38.

The half-life for radioactive decay of ¹⁴C is 5730 years. A wood sample contains only 80% of the ¹⁴C. The age of the wood sample would be-
1. 1898 years
2. 1765 years
3. 1931 years
4. 1860 years

39.

The following mechanism has been proposed for the exothermic catalyzed complex reaction
$A + B ⇌_{fast}^{slow} IAB \overset{k_{1}}{\to} AB + I \overset{k_{2}}{\to} P + A$
If $k_{1}$ is much smaller than $k_{2}$ , the most suitable qualitative plot of potential energy (P.E.) versus reaction co-ordinate (R.C.) for the above reaction
(1)
(2)
(3)
(4)

40.

Consider the reaction.

The rate constant for two parallel reactions were found to be $10^{- 2} {dm}^{3} {mol}^{- 1} s^{- 1}$ and $4 \times 10^{- 2} {dm}^{3} {mol}^{- 1} s^{- 1}$ . If the corresponding energy of activation of the parallel reaction are 100 and 120 kJ/mol respectively, The net energy of activation $(E_{a})$ of A is:
(1) 150 kJ/mol
(2) 320 kJ/mol
(3) 116 kJ/mol
(4) 220 kJ/mol

41.

Select the correct option based on the statements below:

Statement 1:	The overall order of a reaction is the sum of the powers of all the reactants in the rate expression.
Statement 2:	Examples of higher-order reactions (order > 2) are abundant.

1.	Both Statement 1 and Statement 2 are true.
2.	Both Statement 1 and Statement 2 are false
3.	Statement 1 is true, but Statement 2 is false.
4.	Statement 1 is false, but Statement 2 is true.

42.

For study in chemical kinetics, the following relationship is observed
In K (sec^-1) = 12.4 - $\frac{800}{T}$
the activation energy(in cal) of the reaction will be:
1. 2.303 x 8.314 x 800
2. 2.303 x 800
3. 8.314 x 800
4. 2 x 800

43.

The rate constant of the given reaction-
R(g) $\xrightarrow[]{\Delta }$ 2P(g) is 2.48 × 10^–4 s^–1.
A 1 : 1 molar ratio of R to P in the reaction mixture is attained after:
1. 32 min
2. 27.3 min
3. 20 min
4. 0 min

44.

The hydrolysis of ester is alkaline medium is a
1. 1st order reaction with molecularity 1
2. 1st order reaction with molecularity 2
3. 2nd order reaction with molecularity 1
4. 2nd order reaction with molecularity 2

45.

$The reaction A (g) \overset{}{\to} B (g) + 2 C (g) is$
$a first order reaction with rate constant$
$2.772 x 10^{- 3} s^{- 1} . Starting with 0.1 mole$
$of A in 2 liter vessel, find the concentration$
$of A after 250 \sec when the reaction is$
$allowed to take place at constant pressure$
$at 300 K .$
1. 0.0125 M
2. 0.025 M
3. 0.05 M
4. None of these

46.

$Two first order reaction have half - lives in$
$the ratio 8 : 1 . Calculate the ratio of time$
$intervals t_{1} : t_{2} . The time t_{1} and t_{2} are the$
$time period for (\frac{1}{4}) th and (\frac{3}{4}) th completion .$
1. 1 : 0.301
2. 0.125 : 0.602
3. 1 : 602
4. None of these

47.

$The kinetic data for the given reaction$
$A (g) + 2 B (g) \overset{k}{\to} c (g) is provided in$
$the following table for three$
$experiments at 300 K$

Ex. No.	[A/M]	[B/M]	Initial rate ( $M s e c^{- 1}$ )
1.	0.01	0.01	$6.930 x 10^{- 6}$
2.	0.02	0.01	$1.386 x 10^{- 6}$
3.	0.02	0.01	$1.386 x 10^{- 5}$

$In another experiment starting with initial$
$concentration of 0.5 and 1 M respectively$
$for A and B at 300 K, find the rate of$
$raction after 50 minutes from start of$
$experiment (in M / \sec) .$

1.   $6.93 x 10^{- 4}$ M/sec
2.   $0.25 x 10^{- 7}$ M/sec
3.   $4.33 x 10^{- 5}$ M/sec
4.   $3.46 x 10^{- 4}$ M/sec

48.

Plots showing the variation of the rate constant (k) with temperature (T) are given below. The plot that follows Arrhenius equation is –
1.
2.
3.
4.

49.

For a first order reaction A $\to$ P, the temperature (T) dependent rate constant(k) was found to follow the equation logk = – (2000) + 6.0. The pre-exponential factor A and the activation energy E_a,respectively, are-
1. 1.0 × 10⁶ s^–1 and 9.2 kJ mol^–1
2. 6.0 s^–1 and 16.6 kJ mol^–1
3. 1.0 × 10⁶ s^–1 and 16.6 kJ mol^–1
4. 1.0 × 10⁶ s^–1 and 38.3 kJ mol^–1

50.

The decomposition of a gaseous substance (A) to yield gaseous products (B) and (C)
follows first order kinetics. If initially only (A) is present and 10 minutes after the
start of the reaction the pressure of (A) is 200 mm Hg and that of over all
mixture is 300 mm Hg, then the rate constant for 2A $\to$ B + 3 C is –
1. (1/600) ln 1.25 sec^–1
2. (2.303/10) log 1.5 min^–1
3. (1/10) ln 1.25 sec^–1
4. None of the above

51.

The rate of the simple reaction
2NO+O₂ $\to$ 2NO₂, when the volume of the reaction vessel is doubled –
1. Will grow eight times of its initial rate
2. Reduce to one-eighth of its initial rate
3. Will grow four times of its initial rate
4. Reduce to one-fourth of its initial rate

52.

For the reaction, $2 N O_{2} ⇌_{K_{2}}^{K_{1}} N_{2} O_{4}$ , the rate law for the disappearance of $N O_{2}$ will be
1. $K_{1} {[N O_{2}]}^{2} - K_{2} [N_{2} O_{4}]$
2. $2 K_{1} {[N O_{2}]}^{2} - 2 K_{2} [N_{2} O_{4}]$
3. $2 K_{1} {[N O_{2}]}^{2} - K_{2} [N_{2} O_{4}]$
4. $K_{1} {[N O_{2}]}^{2} - 2 K_{2} [N_{2} O_{4}]$

53.

The following data were obtained during the first-order thermal decomposition of $S O_{2} C l_{2}$ at a constant volume.
SO₂Cl₂(g) → SO₂(g) + Cl₂(g)

Experiment	Time/s	Total pressure/atm
1	0	0.5
2	100	0.6

The rate of the reaction when total pressure is 0.65 atm will be:
1. $7.8$ $\times$ $10^{- 4}$ $s^{- 1}$ $a t m .$
2. $0.8$ $\times$ $10^{- 4}$ $s^{- 1}$ $a t m .$
3. $2.4$ $\times$ $10^{- 2}$ $s^{- 1}$ $a t m .$
4. $6.1$ $\times$ $10^{- 8}$ $s^{- 1}$ $a t m .$

54.

1 mole of a gas changes linearly from its initial state (2 atm, 10 lt) to its final state (8 atm, 4 lt). The maximum rate constant is equal to 20 $s e c^{- 1}$ and the value of activation energy is 40 kJ, assuming that the activation energy does not change in this temperature range. The value of the rate constant, at the maximum temperature that the gas can attain, is:
1. $0.56$ $\times$ $10^{- 3}$ $s e c^{- 1}$
2. $3.16$ $\times$ $10^{- 3}$ $s e c^{- 1}$
3. $1.56$ $\times$ $10^{- 3} s e c^{- 1}$
4. $5.12$ $\times$ $10^{- 3}$ $s e c^{- 1}$

55.

What is the percentage of the reactant molecules crossing over the energy barrier at 325 K?
Given that $∆ H_{325} = 0.12$ $kcal,$ $E_{a (b)} = + 0.02$ $kcal$

1.	80.62 %	2.	85.23 %
3.	89.27 %	4.	None of the above

56.

The gas phase decomposition 2N₂O₅ → 4NO₂ + O₂ follows the first order rate law, K = 7.5 × 10^-3 sec^-1. The initial pressure of N₂O₅is 0.1 atm. The time of decomposition of N₂O₅so that the total pressure becomes 0.15 atm will be -

1.	54 sec	2.	5.4 sec
3.	3.45 sec	4.	34.55 sec

57.

The relationship between temperature and the variance in reaction rate is:

1.		2.
3.		4.

58.

In a reaction, the rate = k[A]¹[B]^-2/3 the order of the reaction is-
1. 1/3
2. 2
3. -1/3
4. Zero

59.

A graph between log $t_{\frac{1}{2}}$ and log a (abscissa), a being the initial
concentration of A in the reaction. For reaction A $\to$ Product, the rate law is :

1.	$\frac{-d A}{d t}=\mathrm{K}$	2.	$\frac{-d A}{d t}=K A$
3.	$\frac{-d A}{d t}=K A^2$	4.	$\frac{-d A}{d t}=K A^3$

60.

Consider a reaction $A(g) \xrightarrow { k=0.1 M m^{-1}}2B(g)$. If initial concentration of A is 0.5 M then select graph.

1.		2.
3.		4.

61.

Listed in the table are forward and reverse rate constants for the reaction
2N0(g) $⇌$ $N_{2}$ (g) + $O_{2}$ (g)

Temperature (k)	$K_{f} (M^{- 1} S^{- 1})$	$K_{b} (M^{- 1} S^{- 1})$
1400	0.29	1.1 $\times 10^{6}$
1500	1.3	1.4 $\times 10^{- 5}$

Select the correct statement :
1. Reaction is exothermic and value of equilibrium constant ( $K_{e q}$ ) at 1400 K is 3.79x $10^{- 6}$
2. Reaction is endothermic and value of $K_{e q}$ at 1400 K is 2.63x $10^{5}$
3. Reaction is exothermic and value of $K_{e q}$ at 1400 K is 2.63 X $10^{5}$
4. Reaction is endothermic and value of $K_{e q}$ at 1500 K is 9.28 x $10^{4}$

62.

A first-order reaction is 15 % completed in 20 minutes. The amount of time required to complete 60 % of the reaction is:

1.	112.8 min	2.	120.7 min
3.	100.4 min	4.	140.7 min

63.

The plot of log k vs $\frac{1}{T}$ helps to calculate :
1. Energy of activation.
2. Rate constant of reaction.
3. Order of the reaction.
4. Energy of activation as well as the frequency.

64.

In the following reaction: XA $\to$ YB $\log [\frac{- d (A)}{dt}] = \log [\frac{- d (B)}{dt}] + 0 .3$ where the -ve sign indicates the rate of disappearance of the reactant. Then X: Y is
1. 1:2
2. 2:1
3. 3:1
4. 3:10

65.

A gaseous reaction A₂(g) → B(g) + $\frac{1}{2} C$ (g) shows increase in pressure from 100 mm to 120 mm in 5 minutes. The rate of disappearance of A₂will be :

1.	4 mm min^-1	2.	8 mm min^-1
3.	16 mm min^-1	4.	2 mm min^-1

66.

Half-life is independent of the concentration of a reactant. After 10 minutes, the volume of N₂ gas is 10 L and after complete reaction, it is 50 L. Hence, the rate constant is:
1. $\frac{2.303}{10}$ log 5 min^-1
2. $\frac{2.303}{10}$ log 1.25 min^-1
3. $\frac{2.303}{10}$ log 2 min^-1
4. $\frac{2.303}{10}$ log 4 min^-1

67.

For a first-order reaction A $\to$ Products, the rate of reaction at [A] = 0.2 M is 1.0 x 10^-2 mol litre^-1min^-1. The half-life period for the reaction will be:

1.	832 sec	2.	440 sec
3.	416 sec	4.	14 sec

68.

Rate constant of reaction can be expressed by Arrhenius equation as,
$K = A e^{\frac{- E_{a}}{R T}}$
In this equation, $E_{a}$ represents:
1. the energy above which all the colliding molecules will react
2. the energy below which colliding molecules will not react
3. the total energy of the reacting molecules at a temperature, T
4. the fraction of molecules with energy greater than the activation energy of the reaction

69.

For a given reaction, the presence of a catalyst reduces the energy of activation by 2 kcal at 27 ^oC. The rate of reaction will be increased by:
1. 20 times
2. 14 times
3. 28 times
4. 2 times

70.

How much faster would a reaction proceed at 25°C than at 0°C if the activation energy is 65 kJ?
1. 2 times
2. 16 times
3. 11 times
4. 6 times

71.

In the Arrhenius equation K = Ae^-E_a/RT, the quantity e^-^E_a^/k^T is referred as:
1. Boltzmann factor.
2. Frequency factor.
3. Activation factor.
4. None of the above.

72.

For an exothermic chemical process occurring in two steps as;
(i) A+B $\to$ X(Slow)
(ii) X $\to$ AB (Fast)
The progress of the reaction can be best described by:

1.		2.
3.		4.	All of the above.

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1.	\(2.726 \times 10^{-5} \mathrm{~min}^{-1}\)	2.	\(2.276 \times 10^{-5} \mathrm{~min}^{-1}\)
3.	\(2.216 \times 10^{-5} \mathrm{~min}^{-1}\)	4.	None of the above

1.	\(\mathrm{s}^{-1}\)	2.	\(\mathrm{L} \mathrm{mol}^{-1} \mathrm{~s}^{-1}\)
3.	\(\mathrm{mol} \mathrm{L}^{-1} \mathrm{~s}^{-1}\)	4.	\(\mathrm{L}^2 \mathrm{~mol}^{-2} \mathrm{~s}^{-1}\)

(a)	\(\ln\dfrac{A}{k}=\dfrac{E_a}{R T}\)
(b)	\(\dfrac{d \ln k}{d T}=\dfrac{E_a}{R T^2}\)
(c)	\(\log A=\log k+\dfrac{E_a}{2.303 R T}\)
(d)	\(\log \left(-\dfrac{E_a}{R T}\right)=\dfrac{k}{A}\)

(i)	The thermal decomposition of HI on a gold surface follows a zero-order reaction.
(ii)	Instantaneous rate = \(\operatorname{limit}_{t \rightarrow 0} \frac{\Delta C}{\Delta t}\)
(iii)	The rate of 1^st order reaction is proportional to the first power of the concentration of the reactant.
(iv)	Radioactive reaction follows 1^storder kinetics.

1.	\(\frac{-d A}{d t}=\mathrm{K}\)	2.	\(\frac{-d A}{d t}=K A\)
3.	\(\frac{-d A}{d t}=K A^2\)	4.	\(\frac{-d A}{d t}=K A^3\)

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