This preview shows page 1. Sign up to view the full content.
Unformatted text preview: __F 13___________ 9. The decomposition of hydrogen peroxide to molecular oxygen and water is a first-order
reaction. If it takes 8.0 hrs for the concentration of H2O2 to decrease from 0.80 M to 0.40 M, how
many hours are required for the concentration to decrease from 0.60 M to 0.15 M? (10 pts)
Some useful equations:
[A]t = -kt + [A]o Integrated First –Order rate law
1/[A]t = kt + 1/[A]o ln[A]t = -kt + ln[A] H2O2(aq) ⇄ H2O(l) + O2(g)
First solve for k: Solve for time: 10. Rate constants for the reaction of NO2(g) + CO(g) → NO(g) + CO2(g) are 1.3 M-1s-1 at 700 K
and 23.0 M-1s-1 at 800 K. Calculate the activation energy for this reaction in kJ/mol. (10 pts) 2.87(8.314 J/molK) = (1.79 x 10-4)Ea
Ea = 133784 J/mol = 134 kJ/mol 11. Extra Credit. Predict the effect on the following equilibrium when a catalyst is added into the
reaction mixture. (5 pts)
NO2Cl(g) + NO(g) ⇄ NOCl(g) + NO2(g)
A catalyst will cause the system to reach equilibrium faster but has no effect on the equilibrium. Chemistry 102 Exam 1...
View Full Document