Really hoping for solutions since I’m having a hard time with this. Pls. skip if unsure or not willing to answer the subitems (these are all connected for one item). Thanks in advanced. A kinetics experiment was performed for the formation of a novel compound, UNO, from its reactants, Chemicals G, R, A, D, and E. The first six runs (Runs 1-6) were all performed at 301 K, while the next two runs (Runs 7-8) at varying temperatures. These are tabulated in the table shown below. Table 1. Reaction rate for the reaction of the different chemicals at a given concentration at 301 K.
Really hoping for solutions since I’m having a hard time with this. Pls. skip if unsure or not willing to answer the subitems (these are all connected for one item). Thanks in advanced.
A kinetics experiment was performed for the formation of a novel compound, UNO, from its reactants, Chemicals G, R, A, D, and E. The first six runs (Runs 1-6) were all performed at 301 K, while the next two runs (Runs 7-8) at varying temperatures.
These are tabulated in the table shown below.
Table 1.
| Run | [G], M | [R], M | [A], M | [D], M | [E], M | Rate, M/s |
| 1 | 0.80 | 0.01 | 0.20 | 0.50 | 2.00 | 0.180 |
| 2 | 0.80 | 0.02 | 0.20 | 0.50 | 0.02 | 3.54 x 10-3 |
| 3 | 0.80 | 0.01 | 0.20 | 0.50 | 0.02 | 1.80 x 10-3 |
| 4 | 0.80 | 0.01 | 0.60 | 0.50 | 0.02 | 1.80 x 10-3 |
| 5 | 1.20 | 0.01 | 0.20 | 0.50 | 0.02 | 4.02 x 10-3 |
| 6 | 0.80 | 0.01 | 0.20 | 0.15 | 0.02 | 1.95 x 10-2 |
a. Calculate the rate order of each chemical and overall rate order of the reaction. Use only 2 runs per reagent to determine the rate order.
b. Write the overall rate law expression for the formation of UNO.
c. Calculate the rate constant of the reaction with proper units.
Table 2. Rate constants of reactions held at different temperatures
| Run | Rate Constant | Temperature, K |
| 7 | 1.08 x 10-1 | 277 |
| 8 | 4.66 x 101 | 320 |
d. Using the data from the reactions at 301 K and the data in Table 2, calculate the activation energy in kJ/mol and the Arrhenius constant. With the equation of the line and r2 value.
e. A chemistry student repeated the same kinetics experiment. However, he stirred the solution in Run 1. What do you think is the effect of this error in the reaction rate of solution in Run 1?
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