A room has a volume of 50 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 26°C? R = 0.082 L⋅atm/mol⋅K A)180 kg B)42 kg C)59 kg D)30 kg E)23 kg

Question

Quizplus · Accepted Answer

We can use the ideal gas law to solve for the mass of the air in the room:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

First, we need to convert the volume from m3 to L:

50 m3 = 50,000 L

Next, we can solve for the number of moles of air:

n = PV/RT

= (1.0 atm)(50,000 L)/(0.082 L⋅atm/mol⋅K)(299 K)

= 2073 mol

Finally, we can calculate the mass using the molecular mass:

mass = n x molecular mass

= 2073 mol x 29 g/mol

= 60,117 g = 59 kg (to two significant figures)

Therefore, the best choice is C, 59 kg.

A Room Has a Volume of 50 M3 and Is

A Room Has a Volume of 50 M³ and Is