Olympic cyclists fill their tires with helium to make them lighter. Assume the volume of the tire is 860 mL, that is filled to a total pressure of 120 psi, and that the temperature is 26°C. Also assume an average molar mass for air of 28.8 g/mol. Calculate the mass of the air in an air-filled tire? Calculate the mass of helium in a helium-filled tire? What is the mass difference between the two?

Question
Asked Oct 20, 2019

Olympic cyclists fill their tires with helium to make them lighter. Assume the volume of the tire is 860 mL, that is filled to a total pressure of 120 psi, and that the temperature is 26°C. Also assume an average molar mass for air of 28.8 g/mol. Calculate the mass of the air in an air-filled tire? Calculate the mass of helium in a helium-filled tire? What is the mass difference between the two? 

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Expert Answer

Step 1

First, the moles of air present in ti...

PV nRT
PV
n
RT
Given V 860mL = 0.860L
P 120 psi 8.16atm
T 26°C 299K
Molar mass of air = 28.8 g/mol
8.16atm x 0.860L
n =
0.08205 L.atm/K.mol x 299K
=0.286 moles
Air Mass 0.286 moles x 28.8 g/mol
8.24 g
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PV nRT PV n RT Given V 860mL = 0.860L P 120 psi 8.16atm T 26°C 299K Molar mass of air = 28.8 g/mol 8.16atm x 0.860L n = 0.08205 L.atm/K.mol x 299K =0.286 moles Air Mass 0.286 moles x 28.8 g/mol 8.24 g

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