At STP conditions, \( 11 \mathrm{~g} \mathrm{of} \mathrm{SO}_{2} \) has a volume of \( \begin{array}{l}3.8 \mathrm{~L} \\ 0.0076 \mathrm{~L} . \\ 250 \mathrm{~L} . \\ 22 \mathrm{~L} \\ \text { Submit Request Answer }\end{array} \)

At standard temperature and pressure (STP), 1 mole of a gas occupies approximately 22.4 liters. Given that the molar mass of sulfur dioxide (SO₂) is about 64 g/mol, you can determine the number of moles in 11 g of SO₂ by dividing 11 g by 64 g/mol, which equals approximately 0.171 moles. Multiplying this by the volume of one mole at STP gives you an approximate volume of 3.84 liters. So, 11 g of SO₂ indeed occupies around 3.8 liters at STP. Understanding gas behavior at STP is essential in various fields, including chemistry and environmental science. For example, environmental scientists use this knowledge to calculate pollutant levels in the air and to model how gases disperse in the atmosphere. Similarly, in the chemical industry, knowing how gases behave under standard conditions helps in designing efficient chemical reactors and refining processes.