Sec. 11.1-11.3
Supplemental Instruction
Iowa State University / Leader: / Emily M
Course: / Chem 167
Instructor: / Burnett
Date: / 12/2/13
- In what region of the atmosphere is ozone considered a pollutant? In what region is it considered beneficial?
- Ammonia can react with oxygen to produce nitric oxide and water.
4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g)
If the rate at which ammonia is consumed in a laboratory experiment is 4.23x10-4 mol/Ls, at what rate is oxygen consumed? At what rate is NO produced? At what rate is water vapor produced?
- A gas, AB, decomposes and the volume of B2 produced is measured as a function of time, t. The data obtained are as follows:
Time (min)08.315.419.0
Volume (L)04.28.611.5
What is the average rate of production of B2 for the first 8.3 min? For the first 19 min?
- A reaction has the experimental rate equation Rate = k [A]2. How will the rate change if the concentration of A is tripled? If the concentration of A is halved?
- For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order?
- Rate = k [X][Y][Z]
- Rate = k [X]2[Y]1/2[Z]
- Rate = k [X]1.5[Y]-1
- Rate = k [X]/[Y]2
- The hypothetical reaction, A + B C, has the rate law:
Rate = k [A]x[B]y
When [A] is doubled and [B] is held constant, the rate doubles. But the rate increases fourfold when [B] is doubled and [A] is held constant? What are the values of x and y?
- The following experimental data were obtained for the reaction of NH4+ and NO2- in acid solution.
NH4+(aq) + NO2-(aq) N2(aq) + 2 H2O(l)
[NH4+] (mol/L) / [NO2-] (mol/L) / Rate = Δ[N2]/ Δt (mol/Ls)0.0092 / 0.098 / 3.33x10-7
0.0092 / 0.049 / 1.66x10-7
0.0488 / 0.196 / 3.51x10-6
0.0249 / 0.196 / 1.80x10-6
Determine the rate law for this reaction, and calculate the rate constant.