For the reaction, \(2 A+B \rightarrow 3 C+D\)

An incorrect expression for the rate of reaction is:

1.	\(-\frac{d[C]}{3} d t \)	2.	\(-\frac{d[B]}{d t} \)
3.	\(\frac{d[D]}{d t} \)	4.	\(-\frac{d[A]}{2 d t}\)

At 400 K, the energy of activation of a reaction is decreased by 0.8 kcal in the presence of a catalyst. As a result, the rate will be:

A first-order reaction was started with a decimolar solution of the reactant. After 8 minutes and 20 seconds, its concentration was found to be M/100. The rate constant of the reaction will be:

1. $4.6$ $\times$ ${10}^{-3}se{c}^{-1}$                                      

2. $16.6$ $\times$ ${10}^{-3}$ $se{c}^{-1}$

3. $24.6$ $\times$ ${10}^{-3}$ $se{c}^{-1}$                                   

4. $40.6$ $\times$ ${10}^{-3}$ $se{c}^{-1}$

Given the following reaction:
N₂O₅   as   N₂O₅   ⇌ 2NO₂ + (1/2)O₂
The values of rate constants for the above reaction are 3.45 × 10^-5 and 6.9 × 10^-3 at 27 ^oC and 67 ^oC respectively. The activation energy for the above reaction is : 

1. $102$ $\times {10}^2$ $J$ $$ $$                                    

2. $488.5$ $kJ$

3. $112$ $J$ $$                                             

4. $112.5$ $kJ$

In a first-order reaction A $\to$ products, the concentration of the reactant decreases to 6.25 % of its initial value in 80 minutes. The value of the rate constant, if the initial concentration is 0.2 mole/litre, will be:

1. $2.17$ $\times$ ${10}^{-2}$ $mi{n}^{-1}$

2. $3.46$ $\times$ ${10}^{-2}$ $mi{n}^{-1}$

3. $3.46$ $\times$ ${10}^{-3}mi{n}^{-1}$

4. $2.16$ $\times$ ${10}^{-3}$ $mi{n}^{-1}$

The rate constant, the activation energy, and the Arrhenius parameter of a chemical reaction at 25°C are 3.0×10^-4 s^-1, 104.4 kJ mol^-1 and 6.0×10¹⁴s^-1 respectively.
The value of the rate constant as T → ∞ will be:

1. 2.0 × 10¹⁸ s^-1                                                  

2. 6.0 × 10¹⁴ s^-1

3. $\infty$                                                                   

4. 3.6 × 10³⁰ s^-1

The kinetic data for the reaction: 2A + B₂ → 2AB are as given below

The order of reaction with respect to A and B₂ is, respectively:

The half-life period for a first-order reaction is 20 minutes. The time required to change the concentration of the reactants from 0.08 M to 0.01 M will be:

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

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: