upi sp a Wseh पSK 359.2mL Charles law Va b. The new pressure of a gas when it expands to 1.25L when originally 235mL and 5.34atm. Gas Law: Solve for the Unknown: 5.34x ,235 Bay les law Parl.00 atm 125 - If 23.4grams of Argon is at a volume if1.35L, what volume will the same mass of Cl2 aas take up given that all other conditions are the same? (hint for this one-compare moles) Gas Law: Solve for the Unknown: If 464mL of an ideal gas is at 27°C and 1.05atm, what will be new volume at STP? Gas Law: Solve for the Unknown: = 2.94g of H2 and 2.34g of He are trapped in 2.65L container at standard ture. Determine the.... H2: Mass 294 1.47nsl
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
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