Which one of the following statements for the order of a reaction is incorrect?

1. Order is not influenced by stiochiometric coefficient of the reactants.

2. Order of reaction is sum of power to the concentration terms of reactants to express the rate of reaction.

3. Order of reaction is always whole number.

4. Order can be determined only experimentally.

 

Half-life period of a first order reaction is 1386s. The specific rate constant of the reaction

is

1. 5.0 x 10^-3s^-1

2. 0.5 x 10^-2s^-1

3. 0.5 x 10^-3s^-1

4. 5.0 x 10^-2s^-1

For the reaction, N₂ + 3H₂ $\to$2NH₃, if d[NH₃]/dt = 2x10^-4 mol L^-1s^-1, the value of -

d[H₂]/dt would be 

1. 3x10^-4 mol L^-1s^-1

2. 4x10^-4 mol L^-1s^-1

3. 6x10^-4 mol L^-1s^-1

4. 1x10^-4 mol L^-1s^-1

If a first-order reaction reaches 60% completion within 60 minutes, approximately how much time would it take for the same reaction to reach 50% completion? (log 4=0.60, log 5=0.69)

1. 50 min

2. 45 min

3. 60 min

4. 30 min

Consider the reaction

N₂(g) +3H₂(g) $\to$2NH₃(g)

The equality relationship between $\frac{\mathrm{d}\left[{\mathrm{NH}}_3\right]}{\mathrm{dt}}$ and $-\frac{\mathrm{d}\left[{\mathrm{H}}_2\right]}{\mathrm{dt}}$ is:

$$\begin{gathered} 1.<mspace\; width="1em"></mspace>+\frac{\mathrm{d}\left[{\mathrm{NH}}_3\right]}{\mathrm{dt}}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-\frac{1<mspace\; width="1em"></mspace>\mathrm{d}[\mathrm{H}{}_2]}{3<mspace\; width="1em"></mspace>\mathrm{dt}} \\ 2.<mspace\; width="1em"></mspace>+\frac{\mathrm{d}\left[{\mathrm{NH}}_3\right]}{\mathrm{dt}}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-\frac{2<mspace\; width="1em"></mspace>\mathrm{d}\left[{\mathrm{H}}_2\right]}{3<mspace\; width="1em"></mspace>\mathrm{dt}} \\ 3.<mspace\; width="1em"></mspace>+\frac{\mathrm{d}[\mathrm{NH}{}_3]}{\mathrm{dt}}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-\frac{3<mspace\; width="1em"></mspace>\mathrm{d}\left[{\mathrm{H}}_2\right]}{2<mspace\; width="1em"></mspace>\mathrm{dt}} \\ 4.<mspace\; width="1em"></mspace>+\frac{\mathrm{d}\left[{\mathrm{NH}}_3\right]}{\mathrm{dt}}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-\frac{\mathrm{d}\left[{\mathrm{H}}_2\right]}{\mathrm{dt}} \end{gathered}$$

In a zero order reaction for every 10° rise of temperature, the rate is doubled. If the

temperature is increased from 10°C to 100°C, the rate of the reaction will become

1. 256 times

2. 512 times

3. 64 times

4. 128 times

If the half-life is independent of its initial concentration, then the order of the reaction is:

1. 0 

2. 1

3. 3

4. 2

 For the pseudo first order reaction A + B $\to$ P, when studied with 0.1 M of B is given by -d[A]/dt =k[A] where K = 1.85 x 10⁴ sec^-1. Calculate the value of rate constant for second order reaction :

(1) 1.85 x 10⁴

(2) 1.85 x 10^-4

(3) 1.85 x 10^-5

(4) 1.85 x 10⁵

The activation energy of a reaction is zero. The rate constant of the reaction is :

1. increases with an increase in temperature

2. decreases with a decrease in temperature

3. decreases with an increase in temperature

4. is nearly independent of temperature

For a certain reaction, 10% of the reactant dissociates in 1 hour, 20% of the reactant dissociates in 2 hours, 30% of the reactant dissociates in 3 hours. Then the units of the rate constant is:-

(1) hour^-1

(2) mol L^-1 hr^-1

(3) mol L^-1 sec^-1

(4) mol L sec^-1