For a reaction A$\stackrel{ }{\to }$ Product, rate law is $-\frac{d\left[A\right]}{dt}=K[A{]}_0$. The concentration of A left after time t when $t=\frac{1}{K}$ is:

1. $\frac{[A{]}_0}{e}$

2. $[A{]}_0 \times e$

3. $\frac{[A{]}_0}{e^2}$

4. $\frac{1}{[A{]}_0}$

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.

For the non-stoichiometric reaction 2A + B $\to$ C +D, the following kinetic data were obtained in three separate experiments, all at 298 K.

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