Hydrogen peroxide decomposes spontaneously into water and oxygen gas by a first-

Question

Hydrogen peroxide decomposes spontaneously into water and oxygen gas by a first-order reaction. This is very slow, but adding a small amount of Fe(NO_3)_3 greatly speeds up the reaction. If a 0.564 M solution of peroxide in water is catalyzed with iron, the half-life is 17.3 minutes. What is the concentration of the solution after 12.0 minutes under these conditions? Chlorine atoms react with methane, forming HCl and CH_3. The rate constant for the reaction is 6.0 times 10^7 M^-1s^-1 at 298 K. When the experiment was repeated at 313 K, the rate constant was 7.5 times 10^7 M^-1s^-1. What is the activation energy of the reaction?

Explanation / Answer

3) initial concentration = Ao = 0.564 M

time = t = 12.0 min

rate constant = 0.693 / half life = 0.693 / 17.3

                     = 0.04006 min-1

k = 1/t * ln (Ao / At)

0.04006 = 1/ 12 * ln (0.564 / At)

At = 0.349M

concentration of solution = 0.349 M

Related Questions

Navigate

• Browse (All)
• Browse H
• Subjects

---

---

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