For a first order reaction, the half-life periof is `0.263 k`.
T or F

Answer

To determine whether the statement "For a first-order reaction, the half-life period is 0.263 k" is true or false, we need to analyze the relationship between the half-life and the rate constant for a first-order reaction.

### Step-by-Step Solution:

1. **Understanding Half-Life for First-Order Reactions**:
The half-life (t₁/₂) of a first-order reaction is defined as the time required for the concentration of a reactant to decrease to half of its initial concentration.

2. **Formula for Half-Life**:
The formula for the half-life of a first-order reaction is given by:
\[ t_{1/2} = \frac{0.693}{k} \]
where \( k \) is the rate constant of the reaction.

3. **Analyzing the Given Statement**:
The statement claims that the half-life is \( 0.263 k \). We need to compare this with the established formula for half-life.

4. **Comparing the Two Expressions**:
According to the formula, the half-life is inversely proportional to the rate constant \( k \). The expression \( 0.263 k \) does not match the half-life formula \( \frac{0.693}{k} \).

5. **Conclusion**:
Since \( 0.263 k \) does not equal \( \frac{0.693}{k} \), the statement is false.

### Final Answer:
The statement "For a first-order reaction, the half-life period is 0.263 k" is **False**.

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