For the non-stoichiometric reaction 2A + 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-1 S-1)
0.1 M	0.1 M	$1.2\times {10}^{-3}$
0.1 M	0.2 M	$1.2\times {10}^{-3}$
0.2 M	0.1 M	$2.4\times {10}^{-3}$

 

The rate law for the formation of C is:

1. d[C]/dt = k[ A][B]

2. d[C]/dt = k[ A]²[B]

3. d[C]/dt = k[ A][B]²

4. d[C]/dt = k[ A]

For the reaction N₂ + 3H₂ $\to$ 2NH₃, the rate $\frac{\mathrm{d}\left[{\mathrm{NH}}_3\right]}{\mathrm{dt}}$= 2 x 10^-4 M s^-1 .Therefore, the rate $\frac{-\mathrm{d}\left[{\mathrm{N}}_2\right]}{\mathrm{dt}}$ is given as:

1. 10^-4 Ms^-1

2. 10⁴ Ms^-1

3. 10^-2 sM^-1

4. 10^-4 sM^-1

If 'I' is the intensity of absorbed light and 'c' is the concentration of AB for the photochemical process AB + hv→  AB *, the rate of formation of AB * is directly proportional to:

1. c

2. I

3. I²

4. cI

Which curve represents zero order reaction?

1. 

2. 

3. 

4. 

In a reaction, the rate expression is, rate = K[A][B]^2/3[C]⁰ , the order of the reaction is:

1. 1

2. 2

3. 5/3

4. zero

The rate of a reaction get doubles when the temperature changes from 7°C to 17°C. By what factor will it change for the temperature change from 17°C to 27°C?

1. 1.81

2. 1.71

3. 1.91

4. 1.76

In the Arrhenius equation K = Ae^-E_a/RT, the quantity e^-E_a/kT is referred as:

1. Boltzmann factor.

2. Frequency factor.

3. Activation factor.

4. None of the above.

For the elementary step,

(CH₃)_3.CBr(aq) → (CH₃)₃C⁺ (aq) + Br^- (aq) the molecularity is:

1. zero

2. 1

3. 2

4. cannot ascertained

When ethyl acetate was hydrolysed in pressure of 0.1 N HCl, the rate constant was found to be 5.40 x 10^-5 sec^-1 . But when 0.1 N H₂SO₄ was used for hydrolysis, the rate constant was found to be 6.25 X10^-5sec^-1. Thus, it may be concluded that:

1. H₂SO₄ is stronger than HCI

2. H₂SO₄ is weaker than HCl

3. H₂SO₄ and HCl both have the same strength

4. The data are not sufficient to compare the strength of H₂SO₄ and HCI

The half time of a second order reaction is:

1. Inversely proportional to the square of the initial concentration of the reactants.

2. Inversely proportional to the initial concentration of the reactants.

3. Proportional to the initial concentration of reactants.

4. Independent of the initial concentration of reactants.