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Problem #9: At 210.0 °C a gas has a volume of 8.00 L. What is the volume of this gas at -23.0 °C? Solution: (8.00 L) / (483.0 K) = (x) / (250.0 K) Note how you can have a negative Celsius temperature, but not a negative Kelvin temperature.
- Law Examples and Problems Only
Problem #14: A gas syringe contains 56.05 milliliters of a...
- Charles
Bonus Example: An ideal gas at 7.00 °C is in a spherical...
- Law Examples and Problems Only
Problem #15: 400.0 mL of a gas are under a pressure of 800.0 torr. What would the volume of the gas be at a pressure of 1000.0 torr? (800.0 torr) (400.0 mL) = (1000.0 torr) (x) Bonus Example #1: A particular balloon is designed by its manufacturer to be inflated to a volume of no more than 2.5 liters.
The following practice problems are to master to topics on the ideal gas laws: Boyle’s law, Charles’s law, and Avogadro’s Law, as well as the combined gas law equation. There are examples to work on the Dalton law of partial pressures, the Graham’s law of effusion, and gas stoichiometry.
GAS VOLUMES 1. Volume (dm3) = 24 x moles. vol (dm3) 24 moles. The volume must be in dm3 (there are 1000 cm3 in 1 dm3). vol in dm3 = vol in cm3 1000. Give all answers to 3 significant figures.
Solutions. How many moles of gas (air) are in the lungs of an adult with a lung capacity of 3.9 L? Assume that the lungs are at 1.00 atm pressure and at a body temperature of 40 oC. (Hint: V, P, and T are given. Use the equation PV = nRT where R = 0.082058 ) ∙ % ∙. = 40 oC + 273.15 = 313.15 K.
What volume will the gas occupy at STP? At a certain temperature, molecules of methane gas, CH4 have an average velocity of 0.098 m/s. What is the average velocity of carbon dioxide molecules at this same temperature? Find the relative rate of diffusion for the gases chlorine, Cl2 and ethane, C2H6.
potential volume of the gas contained in a 500.0 mL can at 25°C if it were heated to 54°C. In other words if the can could expand to allow the gas to take up a greater volume, what would be the new volume of the gas when heated as previously described?
