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CHEM1832-Chemistry for Health Science (T1 2025)
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What is the electron configuration of an F– ion?
The rate constant of a first-order process that has a half-life of 225 s is ________ s–1
At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen:
2 N2O5(g) 4 NO2(g) + O2(g)
When the rate of formation of NO2 is 5.5 × 10–4 M/s, the rate of decomposition of N2O5 is ________ M/s
The combustion of ethylene proceeds by the reaction
C2H4(g) + 3 O2(g) 2 CO2(g) + 2 H2O(g)
When the rate of disappearance of O2 is 0.18 M s–1, the rate of appearance of CO2 is ________ M s–1
Consider the reaction A + B C. A series of reactions have been performed using different initial reactant concentrations, and the initial reaction rates have been measured:
| ExperimentNumber | [A](M) | [B](M) | Initial rate(M s–1) |
| 1 | 7 | 6 | 3 |
| 2 | 2.333 | 6 | 0.333 |
| 3 | 2.333 | 2 | 0.111 |
| Where required values in this table are rounded to 3 decimal places |
What is the value of the rate constant k?
The data in the table below were obtained for the reaction:
A + B P
| Experiment Number | [A] (M) | [B] (M) | Initial Rate (M/s) |
| 1 | 0.273 | 0.763 | 2.83 |
| 2 | 0.273 | 1.526 | 2.83 |
| 3 | 0.819 | 0.763 | 25.47 |
The rate law for this reaction is rate = ________
Kinetic data was recorded for a chemical reaction and the graphs below were were produced using the data. Bases off these graphs, determine the overall order of the rate law for this reaction.
Under constant conditions, the half-life of a first-order reaction ________
KI02E01
Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction:
2 NO2 2 NO + O2
In a particular experiment at 255 °C, [NO2] drops from 0.790 M to 0.0125 M in 90.0 s. The rate of disappearance of NO2 for this period is ________ M/s
The peroxydisulfate ion (S2O82–) reacts with the iodide ion in aqueous solution via the reaction:
S2O82–(aq) + 3 I–(aq) 2 SO4(aq) + I3–(aq)
An aqueous solution containing 0.050 M of S2O82– ion and 0.072 M of I– is prepared, and the progress of the reaction followed by measuring [I–]. The data obtained is given in the following table:
| Time (s) | 0.0 | 400.0 | 800.0 | 1200.0 | 1600.0 |
| [I–] (M) | 0.072 | 0.057 | 0.046 | 0.037 | 0.029 |
The concentration of S2O82– remaining at 400 s is ________ M