(a) Calculate the partial pressure (in atm) of O₂ in a 1.000 L sample of air at 95.72 kPa and 25⁰C.
(b) On a very humid day, air can contain as much as 2.00% water by mass at 25⁰C. Calculate the partial pressure of H₂O vapor in 5.000 L of air at 25.0⁰C and 1 atm. The density of air at this temperature is 1.185 g/L.
(b) On a very humid day, air can contain as much as 2.00% water by mass at 25⁰C. Calculate the partial pressure of H₂O vapor in 5.000 L of air at 25.0⁰C and 1 atm. The density of air at this temperature is 1.185 g/L.
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Volume 1L
Temperature = 25⁰C = 298 K
Pressure = 95.72 kPa = 0.944683 atm
In a mixture of ideal gases, each gas has a partial pressure which is the pressure which the gas would have if it alone occupied the volume.
0.2095*0.944683 = 0.2 atm
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Density of air at this temperature is 1.185 g/L.
In 5 liter the mass of air is 5.925 g
2% of this is water
2% of 5.925 is 0.1185g
molar mass of water = 18.01528g /mole
18.01528g has 0.00657 moles
Volume of water is 0.00657* 22.414 = 0.14725998 L at 273 K
Volume at 298 K is = 0.14725998 *298/ 273 = 0.16 L
Percentage of volume = 0.16/5 = 0.032
Partial pressure is 0.032 *1 = 0.032 atmosphere.
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Temperature = 25⁰C = 298 K
Pressure = 95.72 kPa = 0.944683 atm
In a mixture of ideal gases, each gas has a partial pressure which is the pressure which the gas would have if it alone occupied the volume.
0.2095*0.944683 = 0.2 atm
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Density of air at this temperature is 1.185 g/L.
In 5 liter the mass of air is 5.925 g
2% of this is water
2% of 5.925 is 0.1185g
molar mass of water = 18.01528g /mole
18.01528g has 0.00657 moles
Volume of water is 0.00657* 22.414 = 0.14725998 L at 273 K
Volume at 298 K is = 0.14725998 *298/ 273 = 0.16 L
Percentage of volume = 0.16/5 = 0.032
Partial pressure is 0.032 *1 = 0.032 atmosphere.
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