The reaction is first order with respect to cyclopropane with k = 9.2 s-1 at 1000°C.
a) Calculate the half-life of the reaction.

Question

The reaction is first order with respect to cyclopropane with k = 9.2 s-1 at 1000°C.
a) Calculate the half-life of the reaction.

anonymous · Answer

I have to put the equation of half life I guess.

anonymous · Answer

How much of a 3.00 g sample of cyclopropane remains after 0.50 sec at
1000°C

anonymous · Answer

thats the tricky part

xishem · Answer

First calculate the half-life and post that number.

anonymous · Answer

0.074

xishem · Answer

That's right. Now do you happen to know the half-life equation that involves initial amount, final amount, and elapsed time?

anonymous · Answer

I do know the equation

anonymous · Answer

ln[a]=k t1/s+ln(value of given molecule)

xishem · Answer

That's right. Be sure that you have a NEGATIVE sign in front of the kt:$$\ln[A]=-kt+\ln[A]_0$$It's as simple as plugging in the values you know and solving for [A]

anonymous · Answer

but my answer is wrong.

xishem · Answer

I'm getting 0.0302g

anonymous · Answer

first u multiply the value of k with time?

anonymous · Answer

how to calculate it with ln?