The rate constant for the decomposition of NO_2 is 0.255 M^-1 S^-1. Using the un

Question

The rate constant for the decomposition of NO_2 is 0.255 M^-1 S^-1. Using the units of k, first determine if this is a zero^-, first^-, or Second - order reaction. Then answer this question: if a 1.00 L reaction vessel initially contains 1.33 M NO_2, how many moles remain after 4.00 s? What is the activation energy (E_a) for the reaction with the following data? What is the activation energy (Ea) for the reaction with the following data? What is the activation energy (E_a) for a reaction with a rate constant that triples as it is heated from 293K to 308K? Is the following mechanism valid for the overall reaction shown here?

Explanation / Answer

according to units it is second order

take the secon order rate equation

1 /A = kt + 1/A0

A = final concentration

[A0] = intial concentration = 1.33 M

k = rate constant = 0.255 M-1s-1

t = time 4.00 sec

put all these in above equation

1/[A] = 0.255 x 4 + 1/1.33

1/[A] = 1.02 + 0.7518

1/[A] = 1.7718

[A] = 1/1.7718

= 0.56 mol

=

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

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