For a certain reaction a plot of [(c₀-c)/c] against time t, yields a straight line. c₀ and c are concentrations of reactant at t = 0 and t = t respectively. The order of reaction is:

1. 3

2. 0

3. 1

4. 2

Hydrogenation of vegetable ghee at 25⁰C reduces pressure of H₂ from 2 atom to 1.2 atom in 50 minute. The rate of reaction in terms of molarity per second is:

1. 1.09 x 10^-6

2. 1.09 x 10^-5

3. 1.09 x 10^-7

4. 1.09 x 10^-8

A hypothetical reaction, A₂ +B₂ $\to$ 2AB mechanism as given below;

A₂ $\rightleftharpoons$A+ A          ............(Fast)

A+B₂ → AB + B   ............(Slow)

A+ B → AB         ............(Fast)

The order of the overall reaction is:

1. 2

2. 1

3. 1.5

4. zero

Following mechanism has been proposed for a reaction,

2A+B $\to$D+E

A+B$\to$ C+D    ...(Slow)

A+ C$\to$ E         ...(Fast)

The rate law expression for the reaction is:

1. r = K[A]²[B]

2. r=K[A][B]

3. r= K[A]²

4. r= K[A][C]

In gaseous reactions important for the understanding of the upper atmosphere H₂O and O react bimolecularly to form two OH radicals. $∆$H for this reaction is 72kJ at 500 K and E_a is 77 kJ mol^-1, then E_a for the bimolecular recombination of two OH radicals to form H₂O and O is:

1. 3 kJ mol^-1

2. 4 kJ mol^-1

3. 5 kJ mol^-1

4. 7 kJ mol^-1

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