The following reaction was carried out at 300 K.

2SO₂(g)  +  O₂(g) →  2SO₃(g)

The rate of formation of $S{O}_3$ is related to the rate of disappearance of $O_2$  by the following expression:

1. $-\frac{∆\left[O_2\right]}{∆t}=+\frac{1}{2}\frac{∆\left[S{O}_3\right]}{∆t}$                           

2. $-\frac{∆\left[O_2\right]}{∆t}=\frac{∆\left[S{O}_3\right]}{∆t}$

3. $-\frac{∆\left[O_2\right]}{∆t}=-\frac{1}{2}\frac{∆\left[S{O}_3\right]}{∆t}$                           

4. None of the above.

Which of the following rate laws has an over all order of 0.5 for the reaction A + B + C $\to$product ?

1. R=k[A].[B].[C]                                            

2. R=k[A]^0.5[B]^0.5[C]^0.5  

3. R=k[A]^1.5[B]^-1[C]⁰  $$                                

4. R=k[A][B]⁰[C]^0.5

For the system $A_2\left(g\right)+B_2\left(g\right) 2AB\left(g\right),∆H=-80kJ$ If the activation energy for the forward step is 100 kcal/mol.What is the ratio of temperature at which the forward and backward reaction shows the same % change of rate constant per degree rise of temperature ? (1 cal= 4.2 J)

(A) $\sqrt{0.72}$                                                    

(B) $\sqrt{0.84}$

(C) $\sqrt{0.42}$                                                    

(D) $\sqrt{1}$

For a reaction of the type 2A+B $\to$2C, the rate of the reaction is given by $k{\left[A\right]}^2\left[B\right]$. When the volume of the reaction vessel is reduced to 1/4 th of the original volume, the rate of reaction changes by a factor of

(A) 0.25                                                          

(B) 16

(C) 64                                                             

(D) 4

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

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