The total pressure in a flask containing air and ethanol at 25.7C is 878 mm Hg. The pressure of the air in the flask at 25.7C is 762 mm Hg. If the flask is immersed in a water bath at 30.0C, the total pressure is 980 mm Hg.The vapor pressure of ethanol at the new temperature is_________ mm Hg.
I think the problem is flawed. Do you have an answer that you KNOW is right?
To find the vapor pressure of ethanol at the new temperature, we can use the concept of Dalton's Law of Partial Pressures.
According to Dalton's Law of Partial Pressures, the total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas.
In this case, the total pressure in the flask is given as 980 mm Hg, and the pressure of the air in the flask is 762 mm Hg. To find the vapor pressure of ethanol, we need to determine the partial pressure of ethanol.
We know that the total pressure in the flask is the sum of the partial pressures of air and ethanol. Therefore, we can use the following equation:
Total Pressure = Pressure of Air + Vapor Pressure of Ethanol
980 mm Hg = 762 mm Hg + Vapor Pressure of Ethanol
To find the vapor pressure of ethanol, we can rearrange the equation:
Vapor Pressure of Ethanol = Total Pressure - Pressure of Air
Vapor Pressure of Ethanol = 980 mm Hg - 762 mm Hg
Vapor Pressure of Ethanol = 218 mm Hg
Hence, the vapor pressure of ethanol at the new temperature is 218 mm Hg.