Dalton's+Law+R.+Stacey

Dalton ’s Law of Partial Pressure : John Dalton, proposed the atomic theory and also studied gas mixtures. He discovered that the pressure exerted by each gas is independent of the other pressures from other gases present. Sample Problem : Oxygen gas from decomposition of potassium chlorate, KClO3, was collected by water displacement. The barometric pressure and the temperature during the experiment were 731.0 torr and 20˚ C, respectively. What was the partial pressure of oxygen collected? Given = //P//T = //P//atm = 731.0 torr //P// H 2 O = 17.5 torr (vapor pressure of water at 20˚ C) // P // atm = //P// O 2 + //P// H2O Unknown: //P//O2 in torr So, after writing the givens and identifying the unkown, you need to find out what you are trinyg to accomplish. In this case, it is simple subtraction: // P // O 2 = //P//atm - //P// H2O So then you just plug the values in: // P // O 2 = 731.0 torr – 17.5 torr = 713.5 torr
 * The pressure of each gas in a mixture is called the **partial pressure** of that gas.
 * ** Dalton **** ’s law of partial pressure ** says that the total amount of pressure is comprised of the sum of partial pressure components gases.
 * The equation looks like this:   //P//   total   = //P//1 + //P//2 + //P//3 + //P//4 ….

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