A 500. mL sample of hydrogen gas is collected over water at 27 °C. The pressure of the hydrogen and water vapor mixture is 78.5 kPa and the vapor pressure of water at 27 °C is 3.6 kPa. What is the partial pressure of the dry hydrogen gas?
Ptotal = pH2dry + pH2O
You know Ptotal and pH2O, solve for pH2 dry.
Khud Marlo yaar
To find the partial pressure of the dry hydrogen gas, we need to subtract the vapor pressure of water from the total pressure.
The total pressure, given in the problem, is 78.5 kPa.
The vapor pressure of water at 27 °C is 3.6 kPa.
To find the partial pressure of the dry hydrogen gas, we use the equation:
Partial pressure of dry hydrogen gas = Total pressure - Vapor pressure of water
Substituting the values into the equation, we have:
Partial pressure of dry hydrogen gas = 78.5 kPa - 3.6 kPa
Calculating, we find:
Partial pressure of dry hydrogen gas = 74.9 kPa
Therefore, the partial pressure of the dry hydrogen gas is 74.9 kPa.