A physics lecture room at 1.00 atm and 27.0C has a volume of 216 m3. (a) Use the ideal-gas law to estimate the number of air molecules in the room. Assume that all of the air is N2. Calculate (b) the particle density—that is, the number of N2 molecules per cubic centimeter— and (c) the mass of the air in the room.

A physics lecture room at 1.00 atm and 27.0C has a volume of 216 m3. (a) Use the ideal-gas law to estimate the number of air molecules in the room. Assume that all of the air is N2. Calculate (b) the particle density—that is, the number of N2 molecules per cubic centimeter— and (c) the mass of the air in the room.

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Question

A physics lecture room at 1.00 atm and 27.0C has a volume
of 216 m3. (a) Use the ideal-gas law to estimate the number of
air molecules in the room. Assume that all of the air is N2. Calculate
(b) the particle density—that is, the number of N2 molecules per cubic
centimeter—
and (c) the mass of the air in the room.

Definition Definition Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)

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