CHM112 Home Page Reference Materials Homework Assignments Lectures Exams & Quizzes Grades Study Aids URI Home Page


J. W. Hill, R. H. Petrucci, T. W. McCreary, & S. S. Perry General Chemistry, 4th edition.

Problem 13.40.

In the first-order decomposition of dinitrogen pentoxide at 335 K,

N2O5(g) 2NO2(g) + ½O2(g)

if we start with a 2.50-g sample of N2O5 at 335 K and have 1.50 g remaining after 109 s, (a) What is the value of the rate constant k? (b) What is the half-life of the reaction? (c) What mass of N2O5 will remain after 5.0 min?






Answer:

For a first-order reaction, the integrated rate law can be written as

Since the concentration units cancel out, we can work directly in grams for this problem.

(a) [N2O5]0 = 2.50 g, [N2O5]t = 1.50 g, t = 109 s, so

so k = 4.69×10–3 s–1

(b) t½ = 0.693/k = 0.693/4.69×10–3 = 148 s.

(c) t = 5.0 min = 300. s, so