The thermodynamic activity of the molecules of a gas is measured by a factor which is known as the partial pressure. The gases are able to get dissolved, diffused and they react with other molecules of the gases, not on the basis of their concentration but due to their partial pressure.
If the gases are present in the form of a mixture, then each one of it has a particular partial pressure. According to Dalton’s law, the total pressure that is being exerted by an ideal gas is equal to the sum of the partial pressures of the individual gases present in that mixture.
A 500.-mL sample of O2 gas at 24 °C
A mixture contains 5.00 g each of O2, N2
A sample of oxygen gas is saturated with water vapor at 27
Dinitrogen monoxide, N2O, reacts with propane, C3H8, to
A tank contains a mixture of 52.5 g of oxygen
Dalton’s law of partial pressures concerns the properties of mixtures of gases
If a gaseous mixture is made of 2.41 g of
Determine the partial pressure of each gas as shown in this figure
The vapor pressure of water (see Exercise 18.44)
Calculate the indicated quantity for each gas sample. a.
