A sample of hydrogen gas is collected by water displacement at 20.0'C when the atmospheric pressure is 99.8kPa. What is the pressure of the dry hydrogen, if the partial pressure of water vapour is 2.33kPa at that temperature?
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To find the pressure of the dry hydrogen gas, we need to subtract the partial pressure of water vapor from the atmospheric pressure.
Step 1: Convert the temperatures to Kelvin
To convert 20.0°C to Kelvin, add 273.15 to the Celsius temperature:
20.0°C + 273.15 = 293.15 K
Step 2: Subtract the partial pressure of water vapor from the atmospheric pressure
Pressure of dry hydrogen gas = Atmospheric pressure - Partial pressure of water vapor
Pressure of dry hydrogen gas = 99.8 kPa - 2.33 kPa
Pressure of dry hydrogen gas = 97.47 kPa
Therefore, the pressure of the dry hydrogen gas is 97.47 kPa.
To find the pressure of the dry hydrogen gas, we need to subtract the partial pressure of water vapor from the atmospheric pressure.
The atmospheric pressure is given as 99.8 kPa, and the partial pressure of water vapor is given as 2.33 kPa.
To calculate the pressure of the dry hydrogen gas, we subtract the partial pressure of water vapor from the atmospheric pressure:
Dry Hydrogen Pressure = Atmospheric Pressure - Partial Pressure of Water Vapor
Dry Hydrogen Pressure = 99.8 kPa - 2.33 kPa
Dry Hydrogen Pressure = 97.47 kPa
Therefore, the pressure of the dry hydrogen gas is 97.47 kPa.
Ptotal = pH2 + pH2O
Ptotal = 99.8 kpa
pH2O = 2.33 kPa.
PH2 = ?