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

A first-order reaction takes 40 min for 30 % decomposition. The t_1/2 for this reaction will be:

For a certain reaction involving a single reactant, it is found that $C_0\sqrt{T}$ is constant where $C_0$is the initial concentration of the reactant and T is the half-life. What is the order of the reaction ?

(1) 1                                              

(2) Zero

(3) 2                                              

(4) 3

The high temperature ($\approx$ 1200K) decomposition of $C{H}_{3}COOH$(g) occurs as follows as per simultaneous 1st order reactions.

$C{H}_{3}COOH \stackrel{k_1}{\to } C{H}_4+ C{O}_2$

$C{H}_{3}COOH \stackrel{k_2}{\to } C{H}_{2}CO + H_{2}O$

What would be the % of $C{H}_4$by mole in the product mixture (excluding$C{H}_{3}COOH$)?

1. $\frac{50 k_1}{\left(k_1+k_2\right)}$                                            

2. $\frac{100 k_1}{\left(k_1+k_2\right)}$

3. $\frac{200 k_1}{\left(k_1+k_2\right)}$                                           

4. it depends on the time

The reaction , A(g) + 2B(g) C(g) + D(g) is an elementary process. In an experiment, the initial partial pressure of A and B are $P_A$= 0.60 and $P_B$= 0.80 atm. When $P_C$= 0.2atm the rate of reaction relative to the initial rate is

(1) 1/48                                                               

(2) 1/24

(3) 9/16                                                              

(4) 1/6

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:

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:

For the irreversible unimolecular type reaction A $\stackrel{k}{\to }$products in a batch reactor, 80% reactant A($C_{A0} = 1 mole/lit.)$is converted in a 480 second run and conversion is 90% after 18 minute. The order of this reaction is-

(A) 1                                                       

(B) 2

(C) 1/2                                                   

(D) 3/2

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 gas phase decomposition 2N₂O₅ → 4NO₂ + O₂ follows the first order rate law, K = 7.5 × 10^-3 sec^-1. The initial pressure of N₂O₅${\mathrm{ }}_{}$is 0.1 atm. The time of decomposition of N₂O₅ so that the total pressure becomes 0.15 atm will be -