Evolution of the Modern Atomic Theory.

Evolution of the Modern Atomic Theory. - Page Text Content

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1: Charles' Law describes the direct relationship of temperature and volume of a gas. | Charles' Law must be used with the Kelvin temperature scale. This scale is an absolute temperature scale. At 0 K, there is no kinetic energy . According to Charles' Law, there would also be no volume at that temperature.

2: In the mid 1600's, Robert Boyle studied the relationship between the pressure p and the volume V of a confined gas held at a constant temperature. Boyle observed that the product of the pressure and volume are observed to be nearly constant. The product of pressure and volume is exactly a constant for an ideal gas. | Robert Boyle

3: Gay-lussac's Law | According to Gay-Lussac’s law, for a given amount of gas held at constant volume, the pressure is proportional to the absolute temperature.

4: Avogadro's Law | Avogadro's law states that equal volumes of gases at the same temperature and pressure contain the same number of molecules regardless of their chemical nature and physical properties.

5: Combined gas law | The combined gas law combines the three gas laws: Boyle's Law, Charles' Law, and Gay-Lussac's Law. It states the ratio of the product of pressure and volume and the absolute temperature of a gas is equal to a constant.

6: Ideal Gas Law | PV=nRT | A law that describes the relationships between measurable properties of an ideal gas. The law states that P V = n (R) T , where P is pressure, V is volume, n is the number of moles of molecules, T is the absolute temperature, and R is the gas constant (8.314 joules per degree Kelvin). A consequence of this law is that, under constant pressure and temperature conditions, the volume of a gas depends solely on the number of moles of its molecules, not on the type of gas.

7: Dalton's Gas Law | Ptotal = P1 + P2 + P3.... | Dalton's Law explains that the total pressure is equal to the sum of all of the pressures of the parts.

8: Graham's Law of Diffusion | The rate at which gases diffuse is inversely proportional to the square root of their densities.