The oxidation of nitrogen monoxide by oxygen at 25 °C 2NO +O2 NO2 is second orde

Question

The oxidation of nitrogen monoxide by oxygen at 25 °C 2NO +O2 NO2 is second order in NO and first order in O2. Complete the rate law for this reaction in the box below Use the form kJAl]"[B]"... , where ' is understood for m, n (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 2.11x10-3 Ms1 when [NO]- 9.00x10-3 M and [02] = 2.46x10-3 M. From this experiment, the rate constant is

Explanation / Answer

1)

Rate = k [NO]^2[O2]

2)

Rate = k [NO]^2[O2]

2.11*10^-3 M.s-1 = k (9.00*10^-3 M)^2 (2.46*10^-3 M)

k = 95.3 M-2.s-1

Answer: 95.3 M-2.s-1

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

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