Chapter 5, Problem 54
Use the molar volume of a gas at STP to calculate the density (in g>L) of nitrogen gas at STP.
Video transcript
Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose that a can contains a residual amount of gas at a pressure of 755 mmHg and a temperature of 25 °C. What would the pressure be if the can were heated to 1155 °C?
A sample of nitrogen gas in a 1.75-L container exerts a pressure of 1.35 atm at 25 °C. What is the pressure if the volume of the container is maintained constant and the temperature is raised to 355 °C?
Use the molar volume of a gas at STP to determine the volume (in L) occupied by 33.6 g of neon at STP.
What is the density (in g/L) of hydrogen gas at 20.0 °C and a pressure of 1655 psi?
A sample of N2O gas has a density of 2.85 g/L at 298 K. What is the pressure of the gas (in mmHg)?
A 248-mL gas sample has a mass of 0.433 g at a pressure of 745 mmHg and a temperature of 28 °C. What is the molar mass of the gas?