The total pressure in a flask containing air and ethanol at 257C is 800 mm Hg. If the pressure of the air in the flask is 762 mm Hg, the vapor pressure of ethanol is?
I tried doing a relationship of P1 over t1 etc but i don't get the right answer.
Dalton's law of partial pressures says that the total pressure equals the sum of the partial pressures of each gas in the container. If the partial pressure of air is 762 and the total is 800, then the partial pressure of ethanol is >>
38 mm Hg
To find the vapor pressure of ethanol in the flask at 25°C, you can use Dalton's Law of Partial Pressures. According to this law, the total pressure in a mixture of gases is equal to the sum of the partial pressures of each gas.
In this case, the total pressure is given as 800 mm Hg, and the pressure of the air is given as 762 mm Hg. To calculate the vapor pressure of ethanol, we can subtract the pressure of the air from the total pressure.
Vapor pressure of ethanol = Total pressure - Pressure of air
Vapor pressure of ethanol = 800 mm Hg - 762 mm Hg
Vapor pressure of ethanol = 38 mm Hg
Therefore, the vapor pressure of ethanol in the flask at 25°C is 38 mm Hg.