Dalton's+Law+S.+Lindo

Born September 6, 1766 Died July 27, 1844 Was born in Eaglesfield, Cumberland, England He was a meteorologist and chemist Came up with the Atomic Theory ** The partial pressure is the pressure of a one gas in a mixture as if the gas only takes up a container. This law states that the total pressure of a gas mixture is the sum of the partial pressures of the component gases. He believed that the space between gas molecules within the mixture do not influence the motion of other gases. He also believed that a gas sample would be the same whether it was a gas in a container of other gases or a gas in a container by itself. If you lowered the temperature of the gas you will go against the five assumptions of an ideal gas. To determine the partial pressure of a gas you use the ideal gas law equation and the mole fraction relationship. The total pressure is a result of the total number of collisions per unit of wall area in a given time. The equation for partial pressure is: Ptotal=Ph2 + Ph2o
 * //John Dalton//**
 * Dalton’s Law of Partial Pressures:

**Question**: oxygen gas from the decomposition of potassium chlorate, KCIO3, was collected by water displacement. The barometric pressure and the temperature during the experiment were 731.0 torr and 20.0C, respectively. What was the partial pressure of the oxygen collected? **Given:** Pt = Patm = 731.0 torr Ph2o = 17.5 torr ( vapor pressure of the water at 20.0C) Patm = Po2 + Ph2o **Unknown:** Po2 in torr Patm = Po2 + Ph2o 731.0 torr = Po2 + 17.5 torr 731.0 torr – 17.5 torr = Po2 + 17.5 torr – 17.5 torr 731.0 torr – 17.5 torr = Po2
 * // 713.5 torr = Po2  //**

Gas Law Teaching Wiki ~ S. Lindo