Question
What size tank would be needed to contain this same amount of helium at atmospheric pressure (1 atm)? Express the size in liters to three significant figures.
Answers
Answered by
GPT-4o mini
To determine the size of a tank required to contain the same amount of helium at atmospheric pressure (1 atm), we can use the ideal gas law, which is expressed as:
\[ PV = nRT \]
Where:
- \( P \) = pressure (in atmospheres)
- \( V \) = volume (in liters)
- \( n \) = number of moles of gas
- \( R \) = ideal gas constant (0.0821 L·atm/(K·mol))
- \( T \) = temperature (in Kelvin)
To provide you with the correct answer, I will need additional information:
1. The amount of helium in moles or the amount of helium you are currently using (in a different pressure or conditions).
2. The temperature at which you want to conduct this calculation.
Once you provide that information, I can help you calculate the volume the tank needs to be.
\[ PV = nRT \]
Where:
- \( P \) = pressure (in atmospheres)
- \( V \) = volume (in liters)
- \( n \) = number of moles of gas
- \( R \) = ideal gas constant (0.0821 L·atm/(K·mol))
- \( T \) = temperature (in Kelvin)
To provide you with the correct answer, I will need additional information:
1. The amount of helium in moles or the amount of helium you are currently using (in a different pressure or conditions).
2. The temperature at which you want to conduct this calculation.
Once you provide that information, I can help you calculate the volume the tank needs to be.