A solution is made by mixing 45.0 mL of ethanol, C̟H,0, and 55.0 mL of water. ASsuming ideal behavior, what is the vapor pressure of the solution at 20 °C? The relevant values at 20 °C are included in the table. Liquid Density (g/mL) Vapor Pressure, P° (Torr) ethanol 0.789 43.9 water 0.998 17.5 vapor pressure: To:

Octane (C3H₁8) has a vapor pressure of 14.3 torr and a density of 0.703 g/mL. Benzene (CH) has a vapor pressure of 105.0 torr and a density of 0.876 g/mL. Calculate the vapor pressure (in torr) of a solution containing 655 mL of octane and 325 mL of benzene. Assume this solution behaves ideally. torr

An aqueous solution containing glucose has a vapor pressure of 18.6 torr at 25°C. What would be the vapor pressure of this solution at 45°C? The vapor pressure of pure water is 23.8 torr at 25 °C and 71.9 torr at 45°C. Vapor pressure If the glucose in the solution were substituted with an equivalent amount (moles) of NaCl, what would be the vapor pressure at 45°C? Vapor pressure torr torr Submit Answer Try Another Version 5 item attempts remaining

a solution consisting of liquid R and liquid S. The mole fraction of liquid R in the solution is 0.550. At 298 K, the vapor pressure of pure liquid R is 172 mmHg and the vapor pressure of pure liquid S is 60.0 mmHg. Determine the following at 298 K: Vapor pressure of liquid R(mmHg)Vapor pressure of liquid S(mmHg)Total vapor pressure (mmHg)The mole fraction of R in the vapor