Consider the first-order reaction described by the equation propene At a certain

Question

Consider the first-order reaction described by the equation propene At a certain temperature, the rate constant for this reaction is 5.37x 10-4 s-1 Calculate the half-life of cyclopropane at this temperature. Number 1.29 × 1 0 3 Given an initial cyclopropane concentration of 0.00520 M, calculate the concentration of cyclopropane that remains after 1.80 hours. Number Incorrect. The integrated rate equation for a first-order reaction is 3.94 × 10 . 5 | M | | In[A-InA,-kt | where [A] is the concentration at time t, Alo is the initial concentration, and k is the rate constant. O Previous Give Up & View Solution Try Again O Next Exit

Explanation / Answer

1)
Given:
k = 5.37*10^-4 s-1
use relation between rate constant and half life of 1st order reaction

t1/2 = (ln 2) / k
= 0.693/(k)
= 0.693/(5.37*10^-4)
= 1291 s
Answer: 1.29*10^3 s

2)
we have:
[A]o = 0.00520 M
t = 6480.0 s
k = 5.37*10^-4 s-1

use integrated rate law for 1st order reaction
ln[A] = ln[A]o - k*t
ln[A] = ln(0.00520) - 5.37*10^-4*6480
ln[A] = -5.2591 - 5.37*10^-4*6480
ln[A] = -8.7389
[A] = 1.60*10^-4 M
Answer: 1.60*10^-4 M

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.