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 only liquid elements at standard temperature and pressure are bromine (br) and mercury (hg). although, elements caesium (cs), rubidium (rb), francium (fr) and gallium (ga) become liquid at or just above room temperature.

explanation:

lol for the pointsss