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Joe Flanigan

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The gas laws were developed at the end of the 18th century, when scientists began to realize that relationships between pressure , volume and temperature of a sample of gas could be obtained which would hold to approximation for all gases. In Robert Boyle studied the relationship between volume and pressure of a gas of fixed amount at constant temperature. He observed that volume of a given mass of a gas is inversely proportional to its pressure at a constant temperature. Boyle's law, published in , states that, at constant temperature, the product of the pressure and volume of a given mass of an ideal gas in a closed system is always constant. It can be verified experimentally using a pressure gauge and a variable volume container. It can also be derived from the kinetic theory of gases: if a container, with a fixed number of molecules inside, is reduced in volume, more molecules will strike a given area of the sides of the container per unit time, causing a greater pressure.
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Dalton's law also called Dalton's law of partial pressures states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases. Mathematically, the pressure of a mixture of non- reactive gases can be defined as the summation:. The relationship below provides a way to determine the volume-based concentration of any individual gaseous component. Dalton's law is not strictly followed by real gases, with the deviation increasing with pressure.
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