What is the half-life for a first-order reaction that has a rate constant of 2.3 × 10-4 s-1?

Question

What is the half-life for a first-order reaction that has a rate constant of 2.3 × 10-4 s-1?

889 s

Explanation:

The half-life, t1/2, of a first-order reaction is independent of the initial concentration of the reactant, which is why the problem doesn't provide you with one.

In fact, all you need to know in order to calculate the half-life of a first-order reaction is the rate constant,  k, which in your case is equal to

k=7.80⋅10−4s−1

So, the half-life of a first-order reaction can be calculated by using the equation

plug in your values to find

t1/2=ln(2)7.80⋅10-4s−1=∣

Hope this helps!

the correct name for the n3 ion is azide. azide is a polyatomic anion with a -1 charge and is written as n3 -1. it consists of three nitrogen atoms bonded together. hope i . let me know if you need anything else.

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons