Using the Ideal Gas Law, calculate the density in g/L of chlorine gas at 39.5 °C and a pressure of 1.95 atm. (Molar mass of Cl₂ = 70.90 g/mol)

Twenty-five milliliters of liquid nitrogen (density = 0.807 g/mL) is poured into a cylindrical container with a radius of 10.0 cm and a length of 20.0 cm. The container initially contains only air at a pressure of 760.0 mmHg (atmospheric pressure) and a temperature of 298 K. If the liquid nitrogen completely vaporizes, what is the total force (in lb) on the interior of the container at 298 K?

At what temperature in Kelvin does sulfur hexafluoride (SF6) have a density of 0.5550 g/L at a pressure of 0.8210 atm?

Using the Ideal Gas Law, calculate the density of CO2 gas in g/L at 27°C and 0.50 atm pressure.

What is the density of chlorine gas (Cl2) at 0.970 atm and 39.9°C in g/L, given that 1 bar = 0.98692 atm?

What is the density (in g/L) of carbon dioxide gas at STP, given that the molar volume of a gas at STP is 22.4 L/mol?

What is the density of hydrogen sulfide (H₂S) at 1.7 atm and 265 K? Answer in units of g/L.