A sample of O2 gas is collected over water at 23oC at a barometric pressure of 751mm Hg (vapour pressure of water at 23oC is 21mm Hg). The partial pressure of O2 gas in the sample collected is:
A
21mmHg
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B
751mmHg
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C
0.96atm
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D
1.02atm
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Solution
The correct option is C0.96atm Using the Dalton's law P (Total) = Poxygen +Pwater The vapor pressure of water is 21mmHg 751mmHg = Poxygen + 21 mmHg Poxygen = 751 mmHg - 21 mmHg Poxygen =730 mmHg Convert the partial pressure of oxygen in to atmosphere (730 mmHg) (1 atm / 760 mmHg) = 0.96 atm