Problem: How many air molecules are in a 14.0 × 12.0 × 10.0 ft room (28.2 L = 1 ft3)? Assume atmospheric pressure of 1.00 atm, a room temperature of 20.0 °C, and ideal behavior.The ideal gas law describes the relationship among the pressure P, volume V, number of moles n, and absolute temperature T of an ideal gas. Here is the relationship expressed mathematically:PV = nRTwhere R is a proportionality constant. The units of R are determined by the units of pressure and volume used in the equation. When atm is used for pressure and L for volume, the appropriate R value is 0.08206 L ⋅ atm/ mol ⋅ K.

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How many air molecules are in a 14.0 × 12.0 × 10.0 ft room (28.2 L = 1 ft3)? Assume atmospheric pressure of 1.00 atm, a room temperature of 20.0 °C, and ideal behavior.


The ideal gas law describes the relationship among the pressure P, volume V, number of moles n, and absolute temperature T of an ideal gas. Here is the relationship expressed mathematically:

PV = nRT

where R is a proportionality constant. The units of R are determined by the units of pressure and volume used in the equation. When atm is used for pressure and L for volume, the appropriate R value is 0.08206 L ⋅ atm/ mol ⋅ K.

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