# 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?
The text passage contains a chemistry problem that involves calculating the mass difference between helium and air in a bicycle tire under specified conditions. The passage provides the necessary data and a step-by-step solution to find the number of moles of gas, but it does not explicitly state the final mass difference.
single_question_with_answer
Given a text passage, determine:
    1. If it contains a mathematical question (including word problems or calculations)
    2. If an answer to that mathematical question is provided in the text

First, describe the content structure you found in 1-2 sentences.

Then provide your analysis in the following format:
TYPE: <one of the following values>
- NO_QUESTION
- SINGLE_QUESTION
- SINGLE_QUESTION_WITH_ANSWER
- MULTIPLE_QUESTIONS
- MULTIPLE_QUESTIONS_WITH_ANSWERS
system
# 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?
user
The text passage contains a chemistry problem that involves calculating the mass difference between helium and air in a bicycle tire under specified conditions. The passage provides the necessary data and a step-by-step solution to find the number of moles of gas, but it does not explicitly state the final mass difference.

TYPE: SINGLE_QUESTION_WITH_ANSWER