A gas is bubbled through water at a temperature of 30°C and at an atmospheric pressure of
100.2 kPa. What is the pressure of the dry gas?
Ptotal = pH2O + pgas
Ptotal = 100.2 kpa
pH2O--look up vapor pressure H2O at 30 C (in kPa or convert to kPa or convert 100.2 kPa to mm Hg and use pH2O in mm Hg)
Substitute and solve for pgas.
ur wrong its 92
To determine the pressure of the dry gas, we need to consider the relationship between the total pressure, the pressure of the water vapor, and the pressure of the dry gas. This relationship is described by Dalton's Law of Partial Pressures.
According to Dalton's Law, the total pressure is equal to the sum of the partial pressures of the individual gases. In this case, we have water vapor and the dry gas.
To find the pressure of the dry gas, we need to subtract the pressure of the water vapor from the total pressure.
First, let's determine the pressure of the water vapor at 30°C. We can use the water vapor saturation pressure table or a vapor pressure calculator. At 30°C, the saturation pressure of water vapor is approximately 4.24 kPa.
Now, subtract the pressure of the water vapor from the total pressure:
Pressure of the dry gas = Total pressure - Pressure of the water vapor
Pressure of the dry gas = 100.2 kPa - 4.24 kPa
Pressure of the dry gas = 95.96 kPa
Therefore, the pressure of the dry gas is approximately 95.96 kPa.