Zinc metal is added to hydrochloric acid to generate hydrogen gas and is collected over a liquid whose vapor pressure is the same as pure water at 20.0°C (18 torr). The volume of the mixture is 1.7 L, and its total pressure is 0.810 atm.
Determine the partial pressure of the hydrogen gas in this mixture.
To determine the partial pressure of the hydrogen gas, we need to use the ideal gas law equation: PV = nRT.
First, let's convert the total pressure from atm to torr:
0.810 atm * 760 torr/atm = 616.56 torr
We know the total pressure of the mixture is 616.56 torr and the vapor pressure of the liquid is 18 torr. Therefore, the partial pressure of the hydrogen gas is the total pressure minus the vapor pressure of the liquid:
Partial pressure of hydrogen gas = Total pressure - Vapor pressure of liquid
= 616.56 torr - 18 torr
= 598.56 torr
Therefore, the partial pressure of the hydrogen gas in this mixture is 598.56 torr.