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:

1.	324	2.	279
3.	40	4.	100

5 g radioactive substance is taken in 1 L flask. How much substance will be left after 100 years, if half-life of substance in 25 years?

1. 2.5 g

2. 1.5 g

3. 0.625 g

4. 0.3125 g

For an l^st order reaction, k = (8.5×10⁵)e^–15000K/T. The activation energy of the reaction is:  

1. 150 kJ/mol

2.  125 kJ/mol

3.  50 kJ/mol

4.  500 kJ/mol

Select the correct option based on statements below:

The rate constant of a reaction is
3 x 10^-3 mol^-2 L²s^-1. Hence, the order is:

1. 1

2. Zero

3. 2

4. 3

For a zero-order reaction, the initial amount of reaction is 20 g and half-life is 30 minutes. The amount of reactant left after 60 minutes would be:

1. 5 g

2.  10 g

3.  2.5 g

4.  Zero

The rate constant of the given reaction-

R(g) \(\xrightarrow[]{\Delta }\) 2P(g) is 2.48 × 10^–4 s^–1.

A 1 : 1 molar ratio of R to P in the reaction mixture is attained after: 

1. 32 min

2. 27.3 min

3. 20 min

4. 0 min

An increase in the concentration of the reactants of a reaction leads to a change in:

When the temperature of a reaction increases from 300 K to 310 K, the rate of the reaction doubles. What is the activation energy for this reaction?

 \((R=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1} \text { and } \log 2=0.301)\)

For a reaction, activation energy $E_a=0$ and the rate constant at 200 K is    1.6 $\times$ ${10}^6{s}^{-1}$. The rate constant at 400K will be [Given that gas constant, R=8.314 J $K^{-1}$ $mo{l}^{-1}$]

1.  3.2 × 10⁴ s^-1
2. 1.6 × 10⁶s^-1
3. 1.6 × 10³ s^-1
4. 3.2 × 10⁶ s^-1