Calculate the rate constant (with appropriate units) for a first order reaction which is 30.0% complete in 363 s.
What is the value of the half-life of the reaction?
How long will it take for the reaction to go to 95.5% completion?
|Time (days)||[Antibiotic] (mol/L)|
|0||1.24 x 10-2|
|10.||0.92 x 10-2|
|20.||0.68 x 10-2|
|30.||0.50 x 10-2|
|40.||0.37 x 10-2|
This is a first order
Calculate the half-life for the antibiotic. The units should be in days and should be calculated to three significant figures.
If you start with a 1.0 M solution, how long would it take for 22 % of the antibiotic to decompose?
The answer should be in days and should be calculated to three significant figures.
NH4+ (aq) + NO2- (aq) → N2 (g) + H2O (l)
|Experiment||[NH4+]i||[NO2-]i||Initial rate (M/s)|
|1||0.24||0.10||7.2 x 10-4|
|2||0.12||0.10||3.6 x 10-4|
|3||0.12||0.15||5.4 x 10-4|
|4||0.12||0.12||4.3 x 10-4|
First determine the rate law and rate constant.
Under the same initial conditions as in Experiment 4
, calculate [NH4+
] at 284 seconds after the start of the reaction. In this experiment, both reactants are present at the same initial concentration.
The units should be M, and should be calculated to three significant figures.