Given the following sets of values for an ideal gas, calculate the unknown quantity: PRESSURE in Atmospheres, volume in Liters, and Temperature in Kelvin a. P = 785 mm Hg V = ? n = 0.216 mol T = 27.0oC b. P = ? V=665 mL n = 0.0948 mol T = 30.0oC c. At what temperature in oC does 0.398 moles of gas occupy a volume of 11.1 Liters at a pressure of 0.980 atm?
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.
The value of the gas constant, R, is 0.08206 atm*Liters/mole*K
Given the following sets of values for an ideal gas, calculate the unknown quantity: PRESSURE in Atmospheres, volume in Liters, and Temperature in Kelvin
a. P = 785 mm Hg V = ? n = 0.216 mol T = 27.0oC
b. P = ? V=665 mL n = 0.0948 mol T = 30.0oC
c. At what temperature in oC does 0.398 moles of gas occupy a volume of 11.1 Liters at a pressure of 0.980 atm?
d. How many moles of CO2 gas occupy a volume of 757 mL at 10.4 atm and 317 Kelvin?
e. How many grams of CO2 gas are present?
f. What volume of Cl2 gas is occupied by 11.1 grams at 25.0oC and 740 mm Hg?
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