Instructions: Type your answers to the following questions and submit an electronic copy of your completed assignment on Canvas. Points for each question are indicated in front of the question. Name your file as CHEM151_HW10_FirstNameLastInitial
Question 1: Theoretical understanding of reaction kinetics (10pts)
After studying the slides, your notes from lecture and your readings, answer the following questions in 2-3 sentences for each part:
CH3OH + CH3CH2OCOCH3 ⟶ CH3OCOCH3+CH3CH2OH
Question 2 (5pts)
After doing the readings from section 20.1 of Van Loon and Duffy and/or the slides, answer the following questions in 2 sentences for each part:
Question 2 (5x5pts) Basic calculations of rates
H2(g) + Br2(g) à 2 HBr rate = k [H2][Br2]
The hypothetical reaction, A + B à C, has the rate law: Rate = k[A]x[B]y
When [A] is doubled and [B] is held constant, the rate doubles.
The rate increases fourfold when [B] is doubled and [A] is held constant.
What are the values of the exponents x and y?
The following experimental data were obtained for the reaction
2 A + 3 B à C + 2 D
Determine the reaction order for each reactant and the value of the rate constant.
[A] (mol/L) | [B] (mol/L) | Rate = d[C]/dt (mol/L/s) |
0.127 | 0.15 | 0.033 |
0.127 | 0.30 | 0.132 |
0.255 | 0.15 | 0.066 |
Question 3: Basic calculation of half-life for 1st order reactions (15 pts)
Question 4: Using the equation for first order kinetics – exponents/logarithms practice (15pts)
Consider dieldrin, a pesticide in the category of organochlorines. It has a half-life of 934 days. After calculating its reaction rate constant, assuming first order kinetics, calculate the following:
Question 5 – Determining order of reaction and reaction rate from exp data (10pts)
[EXCEL NEEDED] A new organic compound is tested to determine its kinetics and reaction rate. Concentrations of the chemical were measured under the same conditions for 50 hours, starting at a concentration of 14 ppm. The data from the experiment is given below:
time (hr) | C (ppm) |
0 | 14 |
5 | 10.03 |
10 | 6.85 |
15 | 5.3 |
20 | 3.47 |
25 | 1.9 |
30 | 1.71 |
35 | 0.76 |
40 | 1.1 |
45 | 0.27 |
50 | 0.29 |
Question 6 [11.49] Determining order of reaction and reaction rate from exp data (15pts)
[EXCEL NEEDED] The rate of photodecomposition of the herbicide picloram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results, (Data from Hedlund, R.T., Youngston, CR. “The Rates of Photodecomposition of Picloram in Aqueous Systems,” Fate of Organic Pesticides in the Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society, (1972), 159–172.)
time (days) | C (umol L-1) |
0 | 4.14 |
7 | 3.70 |
14 | 3.31 |
21 | 2.94 |
28 | 2.61 |
35 | 2.30 |
42 | 2.05 |
49 | 1.82 |
56 | 1.65 |
Question 7 [11.57] – Arrhenius relationship for k dependence on temperature (5pts)
[EXCEL NEEDED] The table below presents rate constants measured at three temperatures for the following reaction, which is involved in the production of nitrogen oxides in internal combustion engines.
O(g) + N2(g) à NO(g) + N(g)
Determine the activation energy of the reaction in kJ/mol.
k (L/mol/s) | Temperature (K) |
4.4E02 | 2000 |
2.5E05 | 3000 |
5.9E06 | 4000 |
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