If a reaction A + B → C is exothermic to the extent of 30 kJ mol⁻¹ and the forward reaction has an activation energy of 249 kJ mol⁻¹, the activation energy for the reverse reaction in kJ mol^-1 will be:

The correct statement about the rate constant of a reaction is:

The correct statement about X in the below mentioned graph:

Select the correct option based on statements below:

The nature of the reaction represented in the following graph is:

For a reaction A → B, the Arrhenius equation is given as  \(log_{e}k \ = \ 4 \ - \ \frac{1000}{T}\) the activation energy in J/mol for the given reaction will be:

1. 8314

2. 2000

3. 2814

4. 3412

The correct representation of an exothermic reaction is:

1.		2.
3.		4.	Both 1 and 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

For A + B $\to$C + D, $∆$H = -20 kJ mol^-1 , the activation energy of the forward reaction is 85 kJ mol^-1. The activation energy for the backward reaction is…. kJ mol^-1.

If $∆\mathrm{H}$ of a reaction is 100 kJ mol^-1, then the activation energy for the forward reaction must be

1. Greater than 100 kJ mol^-1

2. Less than 100 kJ mol^-1

3. Equal to 100 kJ mol^-1

4. None of the above.