Which of the following statement `(s)` is/are correct

Options

A. The rate constant for the reaction
`2N_(2)O_(5) rarr 4NO_(2)+O_(2)`, is `3.0 xx 10^(-5) s^(-1)`. If the rate is `2.40 xx 10^(-5) mol L^(-1) s^(-1)`, then the concentration of `N_(2)O_(5) = 0.8 mol L^(-1)`.
B. In the intensity equation, `k = A exp (-E//RT)`. A may be termed as the rate constant at very low temperature.
C. If `I` is the intensity of absorbed light and `c` is the concentration of `AB` for the photochemical process `AB+hv rarr AB^(**)`, the rate of formation of `AB^(**)` is diretly proportional to `I^(2)`.
D. The rate constant, the activation energy, and the Arrhenius parameter of a chemical reaction at `25^(@)C` are `3.0 xx 10^(-4) s^(-1)`, `104.4 kJ mol^(-1)`, and `6.0 xx 10^(14) s^(-1)`, respectively. The value of the rate constant as `T rarr oo` is `6.0 xx 10^(14) s^(-1)`.

Explanation

To solve the question regarding which statements are correct, we will analyze each option step by step.

### Step 1: Analyze Option 1
The first option states that the concentration of N2O5 can be calculated given the rate of reaction and the rate constant.

1. **Identify the reaction**: The decomposition reaction of N2O5 is:
\[ 2 N2O5 \rightarrow 4 NO2 + O2 \]
This is a first-order reaction.

2. **Write the rate law**: For a first-order reaction, the rate is given by:
\[ \text{Rate} = k [N2O5] \]
where \( k \) is the rate constant and \([N2O5]\) is the concentration of N2O5.

3. **Substitute the values**: We are given:
- Rate = \( 2.4 \times 10^{-5} \)
- \( k = 3 \times 10^{-5} \)

Plugging these values into the rate equation:
\[ 2.4 \times 10^{-5} = 3 \times 10^{-5} \times [N2O5] \]

4. **Solve for \([N2O5]\)**:
\[ [N2O5] = \frac{2.4 \times 10^{-5}}{3 \times 10^{-5}} = 0.8 \, \text{mol/L} \]

Since the calculated concentration of N2O5 is 0.8 mol/L, **Option 1 is correct**.

### Step 2: Analyze Option 2
The second option claims that the intensity equation can be termed as the rate constant at very low temperatures.

1. **Understand the Arrhenius equation**: The rate constant \( k \) is given by:
\[ k = A e^{-\frac{E_A}{RT}} \]
where \( A \) is the Arrhenius parameter, \( E_A \) is the activation energy, \( R \) is the gas constant, and \( T \) is the temperature.

2. **Evaluate the statement**: The statement incorrectly refers to the intensity equation as the rate constant. The intensity equation does not relate to the rate constant in this manner.

Thus, **Option 2 is incorrect**.

### Step 3: Analyze Option 3
The third option states that the rate of formation of an activated complex is directly proportional to the square of the intensity.

1. **Understand the photochemical process**: The reaction is:
\[ AB + h\nu \rightarrow AB^* \]
The rate of formation of \( AB^* \) is proportional to the intensity \( I \) of the light.

2. **Evaluate the statement**: The rate of formation is directly proportional to \( I \), not \( I^2 \).

Thus, **Option 3 is incorrect**.

### Step 4: Analyze Option 4
The fourth option provides values for the rate constant, activation energy, and Arrhenius parameter and asks if the rate constant at infinite temperature matches the given value.

1. **Given values**:
- \( k = 3 \times 10^{-4} \)
- \( E_A = 104.4 \, \text{kJ/mol} \)
- \( A = 6 \times 10^{14} \, \text{s}^{-1} \)

2. **Use the Arrhenius equation**:
\[ k = A e^{-\frac{E_A}{RT}} \]
At infinite temperature, \( e^{-\frac{E_A}{RT}} \) approaches 1 because \( T \) approaches infinity.

3. **Calculate \( k \)**:
\[ k = 6 \times 10^{14} \times 1 = 6 \times 10^{14} \, \text{s}^{-1} \]

Since the calculated rate constant matches the given value, **Option 4 is correct**.

### Conclusion
The correct options are **Option 1 and Option 4**.