Subjects
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Rate of Reaction | 11 mins | 0 completed | Learn Summary |
Average Rate of Reaction | 18 mins | 0 completed | Learn |
Arrhenius Equation | 16 mins | 0 completed | Learn Summary |
Rate Law | 38 mins | 0 completed | Learn Summary |
Integrated Rate Law | 52 mins | 0 completed | Learn Summary |
Collision Theory | 9 mins | 0 completed | Learn |
Additional Practice |
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Instantaneous Rate of Change |
Energy Diagram |
Catalyst |
Michaelis-Menten Equation |
Reaction Mechanism |
Identifying Reaction Order |
Dinitrogen pentoxide (N2O5) decomposes to NO2 and O2 at relatively low temperatures in the following reaction:
2N2O5(aq) → 4NO2(aq) + O2(g)
This reaction is carried out in a CCl 4 solution at 45°C. The data are described in the table as well as the plots of the concentration versus t, ln concentration versus t, and 1/concentration versus t and results are below. Determine the rate law and calculate the rate constant.
a. Zero order/ 5.3 x10-5 s -1 b. Second order/ 4.8 x 10−4 s −1 M-1 c. First order/5.3 x 10-5 s -1 M-1
d. Second order/ 2.9 x 10−4 s −1 M-1 e. First order/4.8 x 10−4 s −1
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