3. Based on the fact that one mole of any gas at standard temperature and pressure occupies 22.4 liters and contains 6.024 x 10²³ molecules, the following equation can be used to calculate the number of oxygen molecules consumed per minute: (total ml O2 consumed) X (1 liter) X (1 mole) x (6.024 x 10²³ molecules) = molecules O: consumed (total time of experiment) (1000 ml) (22.4 liter) (1 mole) minute Use this equation, and your data, to calculate the rate of O₂ consumption during your experiment, in molecules/minute, at 40 °C.
3. Based on the fact that one mole of any gas at standard temperature and pressure occupies 22.4 liters and contains 6.024 x 10²³ molecules, the following equation can be used to calculate the number of oxygen molecules consumed per minute: (total ml O2 consumed) X (1 liter) X (1 mole) x (6.024 x 10²³ molecules) = molecules O: consumed (total time of experiment) (1000 ml) (22.4 liter) (1 mole) minute Use this equation, and your data, to calculate the rate of O₂ consumption during your experiment, in molecules/minute, at 40 °C.
Biomedical Instrumentation Systems
1st Edition
ISBN:9781133478294
Author:Chatterjee
Publisher:Chatterjee
Chapter11: Instrumentation In Respiration
Section: Chapter Questions
Problem 4P
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