The following reaction is first order in N2O5: N2O5(g) rightarrow NO3(g) + NO2(g

Question

The following reaction is first order in N2O5: N2O5(g) rightarrow NO3(g) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. Calculate the rate of the reaction when [N2O5] = 5.5 Times 10-2M . Express your answer using two significant figures. What would the rate of the reaction be at the same concentration as in part a if the reaction were second order? (Assume the same numerical value for the rate constant with the appropriate units.) Express your answer using two significant figures Zero order? Express your answers using two significant figures.

Explanation / Answer

1)
first order rate law
rate = k?[N?O?]
= 0.053s? ? 5.510?M
= 2.9 * 10? M/s

2)
second order rate law
rate = k?[N?O?]
= 0.053M?s? ? (5.510?M)
= 1.60 *10?? M/s

3) zero order rate law
rate = k
= 0.053Ms?
= 5.310? M/s

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

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