What volume would 1.5 moles of SO2 occupy at 25 °C and 1 bar?

To solve this problem, we can use the Ideal Gas Law, which states that the pressure of a gas times its volume is equal to the number of moles of the gas times the ideal gas constant times the temperature of the gas (in Kelvin). The formula is:

PV = nRT

Where: P = pressure V = volume n = number of moles R = ideal gas constant T = temperature (in Kelvin)

Given: n = 1.5 moles P = 1 bar = 100000 Pa (since 1 bar = 100000 Pascal) T = 25 °C = 298.15 K (since 0 °C = 273.15 K, so 25 °C = 273.15 K + 25 = 298.15 K) R = 8.314 J/(mol.K) (the ideal gas constant)

We need to find V. So, rearranging the formula to solve for V, we get:

V = nRT / P

Substituting the given values into the formula, we get:

V = (1.5 moles * 8.314 J/(mol.K) * 298.15 K) / 100000 Pa

Solving this, we get:

V = 0.037 m³ or 37 liters (since 1 m³ = 1000 liters)

So, 1.5 moles of SO2 would occupy a volume of 37 liters at 25 °C and 1 bar.