32.7 grams of water vapor takes up how many liters at standard temp and pressure (273 K and 100 kPa)

You just need to convert the mass in grams to number of moles and use the ideal gas equation, pV = n RT

where p = 100 kPa, T = 273 K, V is the volume searched, n is the number of moles and R is the unviersal constant of gases = 8.314 J / K * mol

1) Number of moles = mass in grams / molar mass

=> n = 32.7 g / 18.0 g/mol = 1.81667 moles

2) pV = nRT = > V = nRT / p

V = 1.81667 moles * 8.314 (liter*KPa / k*mol) * 273K / (100 KPa) = 41.2 liter

Answer: 41.2 liters