The units of rate constant and rate of reaction are same for: 

1. First order reaction 

2. Second order reaction 

3. Third order reaction 

4. Zero order reaction 

The rate constant is given as \(K = 1.2 \times 10^3~mol^{-1} L^{-1} s^{-1}\), and the activation energy is \(E_a = 2.0 \times 10^2 ~kJ mol^{-1}\). As temperature T approaches infinity, what is the value of the pre-exponential factor (A)?

1. \(2.0 \times 10^2 \mathrm{~mol}^{-1} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\)
2. \(1.2 \times 10^3 \mathrm{~mol}^{-1} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\)
3. \(3.3 \times 10^3 \mathrm{~mol}^{-1} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\)
4. \(2.4 \times 10^3 \mathrm{~mol}^{-1} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\)

The effect of a catalyst in a chemical reaction is to change the 

1. Acivation energy.

2. Equilibrium concentration.

3. Heat of reaction.

4. Final products.

When the concentration of reactant was made 4 times rate of reaction becomes 8 times. The order of reaction with respect to that reactant is 

1. 2

2. 3

3. 1

4. 1.5

The rate constant for a reaction of zero-order in A is 0.0030 mol L^-1 s^-1. How long will it take for the initial concentration of A to fall from 0.10 M to 0.075 M?

1. 8.3 sec

2. 0.83 sec

3. 83 sec

4. 10.3 sec

A first-order reaction is 15 % completed in 20 minutes. The amount of time required to complete 60 % of the reaction is:

Assertion : If the activation energy of reaction is zero temperature will have no effect on the rate constant.

Reason : Lower the activation energy fasten is the reaction.

Assertion : For a reaction $\mathrm{A}\left(\mathrm{g}\right)\to \mathrm{B}\left(\mathrm{g}\right)$

                                 $—{\mathrm{r}}_{\mathbf{e}}=2.5 {\mathrm{P}}_{\mathrm{A}} \mathrm{at} 400\mathrm{K}$

                                 $—{\mathrm{r}}_{\mathbf{e}}=2.5 {\mathrm{P}}_{\mathrm{A}} \mathrm{at} 600\mathrm{K}$

                  activation energy is 4135 J/mol.

Reason : Since for any reaction, values of rate constant at two different temp is same therefore

               activation energy of the reaction is zero.

If concentration are measured in mole/litre and time in minutes , the unit for the rate constant of a $3^{rd}$ order reaction are

(1) $mol li{t}^{-1} mi{n}^{-1}$                                              

(2) $li{t}^2 mo{l}^{-2}mi{n}^{-1}$

(3) $lit mo{l}^{-1}mi{n}^{-1}$                                              

(4) $mi{n}^{-1}$

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.