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

The relationship between temperature and the variance in reaction rate is:

1.		2.
3.		4.

The plot of log k versus $\frac{1}{T}$ is linear with a slope of

(1) $\frac{E_a}{R}$                                                    

(2) $\frac{-E_a}{R}$

(3) $\frac{E_a}{2.303R}$                                             

(4) $\frac{-E_a}{2.303R}$

If a reaction A + B $\to$ C is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy of 70 kJ/mol, the activation energy for the reverse reaction will be:

1. 30 kJ/mol                                       

2. 40kJ/mol

3. 70 kJ/mol                                       

4. 100 kJ/mol