Which of the following is not correct

Options

A. `t_(1//2) = (0.693)/(k)`
B. N = N_(0)e^(-kt)`
C. `(1)/(N) - (1)/(N_(0)) = "ln" kt_(1//2)`
D. None of these

Explanation

To determine which of the statements regarding chemical kinetics is not correct, we will analyze each option provided in the question.

### Step 1: Analyze the first option
The first option states:
\[ T_{1/2} = \frac{0.693}{k} \]
This formula represents the half-life of a first-order reaction, where \( T_{1/2} \) is the half-life and \( k \) is the rate constant. This statement is correct.

### Step 2: Analyze the second option
The second option states:
\[ n = n_0 e^{-kT} \]
This equation represents the concentration of a reactant in a first-order reaction, where \( n \) is the concentration at time \( T \), \( n_0 \) is the initial concentration, and \( k \) is the rate constant. This statement is also correct.

### Step 3: Analyze the third option
The third option states:
\[ \frac{n - n_0}{n_0} e^{kT} \]
This formula is typically used in the context of second-order reactions. However, the correct expression for a second-order reaction is:
\[ \frac{1}{n} - \frac{1}{n_0} = kT \]
This means that the third option is not correctly representing the second-order kinetics.

### Conclusion
Based on the analysis, the incorrect statement is:
**Option 3**: \( \frac{n - n_0}{n_0} e^{kT} \)