A storeroom has a volume of 30 m³ and is filled with air of an average molecular mass of 29 u.What is the mass of the air in the room at a pressure of 1.0 atm and temperature of 22°C? R = 0.082 L · atm/mol · K A) 36 kg B) 1240 kg C) 72 kg D) 700 kg

Question

Quizplus · Accepted Answer

The mass of the air in the room can be calculated using the ideal gas law:PV = nRTwhere P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.We can rearrange this equation to solve for n:n = PV/RTWe can then use the molar mass of the air to convert the number of moles to mass:mass = n * molar massSubstituting the given values into these equations, we get:n = (1.0 atm * 30 m^3) / (0.082 L · atm/mol · K * 295 K) = 120 molmass = 120 mol * 29 g/mol = 3480 g = 3.48 kgTherefore, the mass of the air in the room is 3.48 kg, which is closest to choice A, 36 kg.

A Storeroom Has a Volume of 30 M3 and Is

A Storeroom Has a Volume of 30 M³ and Is