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$\degree$C? R = 0.082 L · atm/mol · K

Question

Quizplus · Accepted Answer

The mass of the air 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 massPlugging in the given values, we get:n = (1.0 atm * 30 m^3) / (0.082 L ·atm/mol ·K * (273.15 K + 22)) = 1240 molmass = 1240 mol * 29 g/mol = 36 kgTherefore, the mass of the air in the room is 36 kg.

A Storeroom Has a Volume of 30 M3 and Is °\degree°

A Storeroom Has a Volume of 30 M³ and Is $\degree$