Final answer:
The molar volume of an ideal gas at 2.00 atm and 546 K can be calculated using the ideal gas law and the combined gas law. The molar volume at STP is 22.4 L/mol, but in this case, the conditions are not at STP. By using the combined gas law, we can calculate the volume of the gas at STP and then use the molar volume to find the molar volume at the given conditions.
Step-by-step explanation:
The molar volume of an ideal gas at 2.00 atm and 546 K can be calculated using the ideal gas law equation. The molar volume is the volume of 1 mole of a gas. At STP (standard temperature and pressure), the molar volume is 22.4 L/mol. However, in this case, the conditions are not at STP. Therefore, we can use the combined gas law to calculate the volume of gas at STP. Once we have the volume at STP, we can use the molar volume of 22.4 L/mol to find the molar volume of the gas at the given conditions.
First, we can calculate the volume at STP using the combined gas law:
(2.00 atm)(V) = (1.93 atm)(22.4 L/mol)
Solving for V, we find:
V = (1.93 atm)(22.4 L/mol) / (2.00 atm) = 21.88 L
Therefore, the molar volume of the gas at 2.00 atm and 546 K is approximately 21.88 L.