Question
Olympic cyclists fill their tires with helium to make them lighter. Calculate the mass of air in an air-filled tire and the mass of helium in a helium-filled tire. What is the mass difference between the two? Assume that the volume of the tire is 855 mL, that it is filled to a total pressure of 125 psi, and that the temperature is 25 C. Also, assume an average molar mass for air of 28.8 g/mol.
Step 1
We know that 1 liter is equal to 1000 milliliters. Therefore, the volume of the tire in liters is given by: \[ V = 855 \, \text{mL} \times \frac{1 \, \text{L}}{1000 \, \text{mL}} = 0.855 \, \text{L} \] Show more…
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Olympic cyclists fill their tires with helium to make them lighter. Calculate the mass of air in an air-filled tire and the mass of helium in a helium-filled tire. What is the mass difference between the two? Assume that the volume of the tire is 855 mL, that it is filled to a total pressure of 125 psi, and that the temperature is 25 °C. Also assume an average molar mass for air of 28.8 g/mol.
Olympic cyclists fill their tires with helium to make them lighter. Calculate the mass of air in an air-filled tire and the mass of helium in a helium-filled tire. What is the mass difference between the two? Assume that the volume of the tire is 855 $\mathrm{mL}$ , that it is filled to a total pressure of 125 $\mathrm{psi}$ , and that the temperature is $25^{\circ} \mathrm{C}$ . Also, assume an average molar mass for air of 28.8 $\mathrm{g} / \mathrm{mol} .$
Olympic cyclists fill their tires with helium to make them lighter. Assume that the volume of the tire is 860 mL , that it is filled to a total pressure of 125 psi , and that the temperature is 23 ∘C. Also, assume an average molar mass for air of 28.8 g/mol. Part A: Calculate the mass of air in an air filled tire. Part B: Calculate the mass of helium in a helium filled tire. Part C: What is the mass difference between the two?
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