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1. The following data pertaining to the reaction between A and B is given with some inferences:

S.No	[A] \(\mathrm{mol} . \mathrm{L}^{-1}\)	[B] \(\mathrm{mol} . \mathrm{L}^{-1}\)	Rate \(\mathrm{mol} . \mathrm{L}^{-1} \mathrm{sec}^{-1}\)
I	\(1 \times 10^{-2}\)	\(2 \times 10^{-2}\)	\(2 \times 10^{-4}\)
II	\(2 \times 10^{-2}\)	\(2 \times 10^{-2}\)	\(4 \times 10^{-4}\)
III	\(2 \times 10^{-2}\)	\(4 \times 10^{-2}\)	\(8 \times 10^{-4}\)

 

a.	The rate constant of the reaction is \(10^{-4}\).
b.	The rate law of the reaction is \(k[A][B]\).
c.	The rate of the reaction increases four times on doubling the concentration of both the reactants.

Mark the correct option among the following:

1.	a, b and c	2.	a and b
3.	b and c	4.	c alone

2. The rate law for the dimerisation of \(NO_2\) is:
 
\(-\frac{\mathrm{d}\left[\mathrm{NO}_2\right]}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{NO}_2\right]^2\)
The value of the specific rate constant, k can be changed by: 
1. Doubling the total pressure on the system. 
2. Doubling the temperature. 
3. Both of (1) and (2) 
4. None of the above. 

3. For the reaction R → P, the concentration of a reactant changes from 0.03 M to 0.02 M in 25 minutes. The average rate of the reaction in M sec^–1 is:
1. 6.67×10^–5 M s^–1
2. 5.67×10^–5 M s^–1
3. 6.67×10^–6 M s^–1
4. 5.67×10^–6 M s^–1

4. \(C(s) + 2 H_2(g) \rightarrow CH_4(g); \Delta H = -74.8~kJ mol^{-1}\)
Which of the following diagrams gives an accurate representation of the above reaction?
[R→reactants; P→products]

1.		2.
3.		4.

5. Effective collisions are known to possess:
A: Energy greater than the threshold energy.
B: Breaking of old bonds in the reactant.
C: Formation of a new bond in the product.
D: High activation energy.
E: Proper orientation.
Choose the correct answer from the options given below:

1.	A, B, C, D only	2.	A, B, C, E only
3.	A, C, D, E only	4.	B, C, D, E only

6. The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of the reaction will be :
(R = 8.314 JK^–1 mol^–1 and log 2 = 0.301)
1. 53.6 kJ mol^–1
2. 48.6 kJ mol^–1
3. 58.5 kJ mol^–1
4. 60.5 kJ mol^–1

7. If the rate constant of a reaction is \(0.03 s^{-1}\), how much time does it take for \(7.2\text { mol L}^{-1}\) concentration of the reactant to get reduced to \(0.9~\text {mol L} ^{-1}?\)
(Given: log 2=0.301)

1.	210 s	2.	21.0 s
3.	69.3 s	4.	23.1 s

8. Which of the following plots is correct for the given reaction?
([P]₀ is the initial concentration of P)

1.		2.
3.		4.

 

9. Order of a reaction, given that the initial concentration of 0.24 M is reduced to 0.12 M in 10 hours and to 0.06 M in 20 hours, is:

1.	Zero order reaction	2.	First order reaction
3.	Second order reaction	4.	Half order reaction

10.

Statement I:	Order is applicable only for elementary reactions whereas molecularity is applicable for both elementary as well as complex reactions.
Statement II:	Order of a reaction is an experimental quantity.

 
In the light of the above statements, identify the correct option:
1. Both Statement I and Statement II are correct
2. Both Statement I and Statement II are incorrect
3. Statement I is incorrect but Statement II is correct
4. Statement I is correct but Statement II is incorrect