Question

The velocity constant for the first order reaction is $6.93 \times 10^{-3}$ min$^{-1}$. Calculate the half-life of this reaction.

Hint:

For first-order kinetics: higher $k$ → shorter half-life, lower $k$ → longer half-life.

Answer 1

Step 1: Formula.
\[ t_{1/2} = \frac{0.693}{k} \] Step 2: Substitution.
\[ t_{1/2} = \frac{0.693}{6.93 \times 10^{-3}} \] \[ t_{1/2} = 100 \, \text{min} \] Conclusion:
The half-life of the given reaction is: \[ \boxed{100 \, \text{minutes}} \]