Integrated Half-life & Arrhenius Equation practice test PDF

Preview

Summary

practice exam...

Description

Chem 4, Dr. La Gattuta E/C HW Integrated Half-life & Arrhenius Eq.

p.1

Name ________________________________________________ IMPORTANT: E/C HW’S must include FORMULAS/PLUG-IN’S & SOLVES AND MUST BE NEATLY DONE OR THEY WILL BE RETURNED WITH NO CREDIT GIVEN

1) When N2O4 decomposes it forms NO2:

N2O4 ----> 2 NO2

If the half-life of this 1st order reaction is 1386 seconds, how much of a 10.0 gram sample would be left after 1500 seconds?

2)

SO2Cl2 (g)

SO2 (g) + Cl2 (g)

SO2Cl2 decomposes in a first order reaction with a half-life of 4.88 x 102 seconds. If the original concentration is 0.20 M, how many minutes will it take to reach 0.020 M?

Chem 4, Dr. La Gattuta E/C HW Integrated Half-Life & Arrhenius Eqs.

p.2

Name ____________________________________________________ 3) What is the half-life in minutes of a reactant that is second order when the initial concentration is .350 M and the rate constant is .0275/M min?

4) a) The decomposition of a certain insecticide in water follows second-order kinetics with a rate constant of 1.25 M-1yr.-1 How long will it take in months for a .0600 M concentration to reach 0.0150 M?

b) What is the half-life for the reaction of the insecticide?

Chem 4, Dr. La Gattuta E/C HW Integrated Half-Life & Arrhenius Eq. Name _________________________________________________________

p.3

6) The half-life of a first-order reaction is found to be 28.25 min. a) What is the rate constant (k) for this reaction?

b) Approximately how long would it take in minutes for 95.0% of the original amount of reactant A to disappear?

c) If the initial concentration of reactant A is 2.50 M, what is the concentration after exactly 3.00 hours?

d) Using the concentration of the reactant at exactly 3.00 hours, calculate the rate of the reaction at this point....