text: # Problem: 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 25 oC. Also, assume an average molar mass for air of 28.8 g/mol.What is the mass difference between the two?
  
  ###### FREE Expert Solution
  
  Calculate the moles of that can occupy the tire:
  
  $\mathbf{PV}\mathbf{=}\mathbf{nRT}\phantom{\rule{0ex}{0ex}}\frac{\mathbf{PV}}{\mathbf{RT}}\mathbf{=}\frac{\mathbf{n}\overline{)\mathbf{RT}}}{\overline{)\mathbf{RT}}}\phantom{\rule{0ex}{0ex}}\overline{)\mathbf{n}\mathbf{=}\frac{\mathbf{PV}}{\mathbf{RT}}}$
  
  T = 25°C +273.15 = 298.15 K
  
  V = 0.860 L
  
  P = 8.6058 atm
  
  n = 0.299 mol ≈ 0.30 mol
  
  Calculate the mass of helium (He) and air:
  
  85% (461 ratings)
  ###### Problem Details
  
  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 25 oC. Also, assume an average molar mass for air of 28.8 g/mol.
  
  What is the mass difference between the two?
explanation: The text extract contains a chemistry problem that involves calculating the mass difference between helium and air in a bicycle tire under specified conditions. The extract includes the problem statement and a detailed solution, which calculates the moles of gas that can occupy the tire and then the mass of helium and air.
distilabel_metadata.content: Evaluate the user given text extract and determine if it contains a math question and optionally and answer to this question.
  
  Output rules:
  
  1. Briefly describe the document and mention if it contains a question or a question and answer.
  2. Finalize the output with: Label: no-question,question,question-and-answer,multiple-question,multiple-question-and-answer
distilabel_metadata.role: system
distilabel_metadata.content: # Problem: 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 25 oC. Also, assume an average molar mass for air of 28.8 g/mol.What is the mass difference between the two?
  
  ###### FREE Expert Solution
  
  Calculate the moles of that can occupy the tire:
  
  $\mathbf{PV}\mathbf{=}\mathbf{nRT}\phantom{\rule{0ex}{0ex}}\frac{\mathbf{PV}}{\mathbf{RT}}\mathbf{=}\frac{\mathbf{n}\overline{)\mathbf{RT}}}{\overline{)\mathbf{RT}}}\phantom{\rule{0ex}{0ex}}\overline{)\mathbf{n}\mathbf{=}\frac{\mathbf{PV}}{\mathbf{RT}}}$
  
  T = 25°C +273.15 = 298.15 K
  
  V = 0.860 L
  
  P = 8.6058 atm
  
  n = 0.299 mol ≈ 0.30 mol
  
  Calculate the mass of helium (He) and air:
  
  85% (461 ratings)
  ###### Problem Details
  
  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 25 oC. Also, assume an average molar mass for air of 28.8 g/mol.
  
  What is the mass difference between the two?
distilabel_metadata.role: user
distilabel_metadata.raw_output_q_a_detector_0: The text extract contains a chemistry problem that involves calculating the mass difference between helium and air in a bicycle tire under specified conditions. The extract includes the problem statement and a detailed solution, which calculates the moles of gas that can occupy the tire and then the mass of helium and air. 
  
  Label: question-and-answer