Answer:
To solve this problem, we need to use the ideal gas law, which states:
PV = nRT
where P is pressure, V is volume, n is the number of moles of gas, R is the universal gas constant, and T is temperature. Rearranging this equation, we get:
n = PV/RT
We can use this equation to find the number of moles of N2O in 112 L at standard temperature and pressure (STP), which is 1 atm and 273 K:
n = (1 atm)(112 L)/(0.0821 L·atm/mol·K)(273 K)
n = 4.40 mol
Next, we can use the molar mass of N2O, which is 44.01 g/mol, to find the mass of 4.40 mol:
mass = (4.40 mol)(44.01 g/mol)
mass = 193.24 g
Therefore, 112 L of N2O at STP would be equivalent to 193.24 g.