Chemistry - The Ideal Gas Law
Determine the number of moles of air present in 1.35 L at 750 torr and 17.0°C.
0.0560
A balloon containing 0.500 mol Ar at 0.00°C and 65.0 kPa pressure is expanded by adding more argon. How many moles of argon are added to bring the sample to a final volume of 60.0 L at 30.0°C and 45.0 kPa? What is the original volume of the gas?
17.5
At 35.0°C and 3.00 atm pressure, a gas has a volume of 1.40 L. What pressure does the gas have at 0.00°C and a volume of 0.950 L?
3.92
What is the temperature in kelvin of a gas if it is allowed to expand from 1.50 L to 4.50 L? The initial temperature is 10.0°C and pressure is constant throughout the change.
849
A sample of N2 gas occupying 800 mL at 20.0°C is chilled on ice to 0.00°C. If the pressure also drops from 1.50 atm to 1.20 atm, what is the final volume of the gas?
932
Which laws can be combined to form the ideal gas law?
Charles's law, Avogadro's law, and Boyle's law
A student uses 0.0821 L• atm/mol • K as the value of the gas constant. What is most likely true about the variables in the ideal gas law?
V has the units of liters, and T has the units of kelvin.
Avogadro's law and Charles's law describe a proportionality of the volume of a gas when the pressure is constant. Which describes the proportionality that allows these laws to be combined when describing a gas?
Volume is directly proportional to moles (Avogadro's law) and to temperature (Charles's law).
Which statement would be the most useful for deriving the ideal gas law?
Volume is directly proportional to the number of moles.
ideal gas law
an equation (PV = nRT) that relates the volume, pressure, absolute temperature, and number of moles of a gas under ideal conditions
Which law relates temperature, pressure, volume, and the number of moles of a gas under perfect conditions?
ideal gas law
ideal gas constant
the constant (given the symbol R) that is used to relate volume, pressure, absolute temperature, and number of moles of a gas in the ideal gas law equation
Avogadro's law
the law that states that the volume of a gas is proportional to the number of moles of the gas when pressure and temperature are kept constant