From the following data , the orders with respect to A, B, C , respectively, are :

[A] (mol/L)	[B] (mol/L)	[C] (mol/L)	rate (M/sec.)
0.2	0.1	0.02	8.08 x 10-3
0.1	0.2	0.02	2.01 x 10-3
0.1	1.8	0.18	6.03 x 10-3
0.2	0.1	0.08	6.464 x 10-2

1. $-1,$ $1,$ $3/2$                                     

2. $-1,$ $1,$ $1/2$

3. $1,$ $3/2,-1$                                     

4. $1,-1,$ $3/2$

The elementary reaction A + B $\to$products has k = 2 × 10^-5 M^-1 s^-1 at a temperature of $\mathrm{27 }°$C. Several experimental runs are carried out using stoichiometric proportion. The reaction has a temperature coefficient value of 2.0. At what temperature should the reaction be carried out if, in spite of halving the concentrations, the rate of reaction is desired to be 50 % higher than in the previous run?

(Given $\frac{\mathcal{l}n6}{\mathcal{l}n\mathrm{2 }}= 2.585)$

1. $\mathrm{47 }°C$                                           

2. $\mathrm{53 }°C$

3. $\mathrm{57 }°C$                                           

4. $\mathrm{37 }°C$

When the temperature of a reaction increases from 27 ^oC to 37 ^oC, the rate increases by 2.5 times. The activation energy in the temperature range will be:

1. 53.6 kJ                                             

2. 12.61 kJ

3. 7.08 kJ                                             

4. 70.8 kJ

For the reaction $R-X+OH \to ROH+$$X^{-}$ The rate is given of

Rate=$5.0\times {10}^{-5}\left[R-X\right]\left[O{H}^{-}\right]+0.20\times {10}^{-5}\left[R-X\right]$ what percentage of R-X Reaction by $S{N}^2$ mechanism when $\left[O{H}^{-}\right]=1.0\times {10}^{-2}M$

1. 96.1%                                                         

2. 3.9%

3. 80%                                                           

4. 20%

The graph that represents a first-order reaction is:

1.		2.
3.		4.

The rate of a reaction increases 4-fold when concentration of reactant is increased 16 times.

If the rate of reaction is 4 × 10^-6 mol L^-1s^-1 when concentration of the reactant is 4 × 10^-4  mol L^-1, the rate constant of the reaction will be : 

1. 2 × 10^-4 m^1/2 L^-1/2 s^-1                            

2. 1 × 10^-2 s^-1

3. 4 × 10^-4 mol^-1/2 L^-1/2 s^-1                         

4. 25 mol^-1L min^-1                              

If ‘a’ is the initial concentration of a substance which reacts according to zero-order kinetics and k is the rate constant, the time for the reaction to go to completion will be:

The decomposition of a gaseous compound yields the following information:

For a given reaction the concentration of the reactant plotted against time gave a straight line with negative slope.

The order of the reaction will be:

1. 3                                                      

2. 2

3. 1                                                      

4. 0

The rate constant of a first-order reaction is typically determined from a plot of:

1. Concentration of reactant vs time t

2. Log (concentration of reactant) vs time t

3. \(\frac{1}{\text { concentration of reactant }} \text { vs time } t\)
4. Concentration of reactant vs log time t