Answer:
1.6 × 10³ s
Explanation:
Let's consider the following generic reaction.
A → B
The rate law is:
[tex]rate=k \times [A]^{m}[/tex]
where,
rate is the reaction rate
k is the rate constant
[A] is the molar concentration of the reactant A
m is the reaction order
When m = 1, we have a first-order reaction. We can calculate the half-life for this reaction using the following expression.
[tex]t_{1/2}=\frac{ln2}{k} =\frac{ln2}{4.3 \times 10^{-4}s^{-1} }=1.6 \times 10^{3}s[/tex]
