NSCI 1321 Lecture Notes - Lecture 7: Van Der Waals Equation, Molecular Mass, Intermolecular Force
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Use the ideal gas law to find moles from a given volume, pressure, and temperature, and vice versa. Dalton found that in a mixture of unreactive gases, each gas behaves as if it were the only gas in the mixture as far as pressure is concerned. Originally (left), flask a contains he at 152 mmhg and flask b contains o2 at 608 mmhg. Flask a is then filled with oil forcing the he into flask b (right). The new pressure in flask b is 760 mmhg. The pressure exerted by a particular gas in a mixture. The sum of the partial pressures of all the different gases in a mixture is equal to the total pressure of the mixture: The mole fraction of a component gas is the fraction of moles of that component in the total moles of gas mixture. The result is a mixture of the gas and water vapor.