NSM12C Useful Equations and constants: PV=nRT ( )
M ⋅P
d g L = wt R⋅T
Worksheet ( 2)
P = g×h×d P1 V1 P2 V2
=
T1
T2
Week 6 R = 0.08206
L ⋅ atm
mol ⋅ K
1mm Hg = 1torr 1 mole = 22.4 L (at STP) 1. Convert 1.25 atm to mm Hg. 2. Calculate the height in meters of a column of liquid glycerol (density = 1.26 g/cm3) required to exert the same pressure as 760 mmHg (d = 13.60 g/cm3). 3. What volume will a balloon occupy at 1.0 atm, if the balloon has a volume of 7.6 L at 3.8 atm? 4. To what volume will a sample of gas expand if it is heated from 50.0∘C and 2.33 L to 500.0°C? 5. What pressure (in atm) will 0.44 moles of CO2 exert in a 2.6 L container at 25°C? 6. A balloon filled with helium gas at 20°C occupies 4.91 L at 1.00 atm. The balloon is immersed in liquid nitrogen at ‐196°C, while the pressure is raised to 5.20 atm. What is the volume of the balloon in the liquid nitrogen? 7. A 0.465 g sample of an unknown compound occupies 245 mL at 298 K and 1.22 atm. What is the molar mass of the unknown compound? 8. How many liters of oxygen are needed to exactly react with 19.8 g of methane at STP? 9. Potassium chlorate decomposed upon heating to for potassium chloride and oxygen. Determine the volume of O2 (at STP) formed when 50.0 g of potassium chlorate (112.55 g/mol) decomposes. 10. A 34.8 mL sample of an unknown, water‐insoluble gas was collected over water at 22.6°C and a barometric pressure of 0.895 atm. When the gas was dried and chilled, it formed 114.6 mg of liquid. What was the molar mass of this substance? [The vapor pressure of water at 22.6°C is 20. mmHg] Page 1 of 1