The unsaturated hydrocarbon butadiene (C4H6) dimerizes to 4-vinylcyclohexene (C8

Question

The unsaturated hydrocarbon butadiene (C4H6) dimerizes to 4-vinylcyclohexene (C8H2). When data collected in studies of the kinetics of this reaction were plotted against reaction time, plots of [C4H6] or In[C4H6] produced curved lines, but the plot of 1/[C4H6] was linear. a. What is the rate law for the reaction? Rate= b. How many half-lives will it take for the [C4H6] to decrease to 3.1% of its original concentration? The relationship of [A]t I[A]0= 0.50^n, where n = number of half-lives. n= Number

Explanation / Answer

By trial and error the reaction follows second order reaction

1/Ct= 1/C0 +kt (Equation for second order reaction)

Hence rate r = k[C4H6]2 .

Given [At]/[A0] = 0.50n

n = ln([At]/[A0])/ln(0.5)

   = ln(0.031)/ln(0.5) = 5.011

Hence it takes ~ five half lives for concentration to reach 3.1% of initial

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

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