Answer :
Final answer:
2.00 mol of helium would fill a 2.00 L container at a temperature of approximately 12.21 Kelvin under standard pressure.
Explanation:
This question is related to the concept of Standard Temperature and Pressure (STP) in chemistry. According to standard conditions, at STP, one mole of an ideal gas has a volume of about 22.4 L. To find the temperature at which 2.00 mol of helium would fill a 2.00 L container, we would make use of the ideal gas law and the conditions of STP.
Step-by-Step Explanation
1. At STP, the molar volume of an ideal gas is 22.4 L/mol.
2. You have 2 mol of helium, so under STP conditions this would occupy 2 mol x 22.4 L/mol = 44.8 L.
3. However, you only have a 2 L container, so we need to find out what temperature we'd require for this volume to shrink to only 2 L under the same pressure (the standard pressure).
4. As the volume is directly proportional to the temperature (according to Charles' Law), we would calculate the new temperature as: (2 L / 44.8 L) x 273.15 K = 12.21 K.
In conclusion, 2.00 mol of helium would fill a 2.00 L container at a temperature of approximately 12.21 K under standard pressure.
Learn more about Standard Temperature and Pressure here:
https://brainly.com/question/29129606
#SPJ11
