According to the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. At STP (Standard Temperature and Pressure), the pressure is 1 atm and the temperature is 273 K.
From the given information, we know that the volume of sulfur dioxide is 36.2 L at STP. Since one mole of any gas occupies 22.4 L at STP, we can convert the volume of sulfur dioxide to moles:
36.2 L / 22.4 L/mol = 1.616 moles of SO2
To convert moles to grams, we need to know the molar mass of sulfur dioxide. Sulfur has a molar mass of 32.07 g/mol, and oxygen has a molar mass of 16.00 g/mol (since there are two oxygen atoms in SO2, we multiply the molar mass of oxygen by 2). Therefore, the molar mass of SO2 is:
32.07 g/mol + 2(16.00 g/mol) = 64.07 g/mol
Finally, we can use the molar mass of SO2 to convert moles to grams:
1.616 moles x 64.07 g/mol = 103.6 g
Rounding to the nearest whole number, we get 104 g of SO2. Therefore, the answer is (d) 104 g.