An average adult has a total lung capacity of 6.0 L. How many total grams of air could be held in the lungs at a pressure of 102 kPa and a normal body temperature of 37° Celsius? (Assume that the average molar mass of air is 29 g/mol.)

Question

Doogie

Chemistry

2 April, 18:55

An average adult has a total lung capacity of 6.0 L. How many total grams of air could be held in the lungs at a pressure of 102 kPa and a normal body temperature of 37° Celsius? (Assume that the average molar mass of air is 29 g/mol.)

+1

Answers (1)

Know the Answer?

Lennon Schmidt · Answer 1

You're able to figure this out by using the ideal gas equation PV=nRT Where R=.08 (L*atm/mol*K) Convert 37 C to Kelvin=310 K and 102 kPa to atm=roughly 1 atm Manipulate the ideal gas equation to n=PV/RT Plug in your values (1 atm * 6 L) / (.08 (L*atm/mol*K) * 310 K) All units should cancel except for mol and you should get. 24 mol. Multiply the molar mass of air by your answer ...24 mol * 29 g/mol moles should cancel and you should get 6.9 g.