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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Table 2. Oxygen consumption in pea seeds respiring at 40 C.
Tube #1 - Live peas
Time (mins)
0
2
4
6
8
10
12
14
16
18
20
Dye Position
.83
.83
.83
.73
.71
.67
.63
.60
57
.55
5
.50
Total ml O₂
consumed
0
0
0
.10
.12
.16
20
.23
26
28
.33
Tube #2 - Heat-killed peas
Dye position
.83
.80
.81
.87
.87
.86
.86
.86
.87
.87
.87
Total ml O₂
consumed
0
.03
.02
.04
.04
.03
.03
.03
.04
.04
.04
Transcribed Image Text:Table 2. Oxygen consumption in pea seeds respiring at 40 C. Tube #1 - Live peas Time (mins) 0 2 4 6 8 10 12 14 16 18 20 Dye Position .83 .83 .83 .73 .71 .67 .63 .60 57 .55 5 .50 Total ml O₂ consumed 0 0 0 .10 .12 .16 20 .23 26 28 .33 Tube #2 - Heat-killed peas Dye position .83 .80 .81 .87 .87 .86 .86 .86 .87 .87 .87 Total ml O₂ consumed 0 .03 .02 .04 .04 .03 .03 .03 .04 .04 .04
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 O₂ 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.
Transcribed Image Text: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 O₂ 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.
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