7. Gases

Consider two containers of gases at the same temperature. One has helium at a pressure of 1.00 atm. The other contains carbon dioxide with the same density as the helium gas. What is the pressure of the carbon dioxide gas sample?

Determine the molecular formula of a gaseous compound that is 49.48% carbon, 5.19% hydrogen, 28.85% nitrogen, and 16.48% oxygen. At 27°C, the density of the gas is 1.5535 g/L and it exerts a pressure of 0.0985 atm.

Consider the following samples of gases:

If the three samples are all at the same temperature, rank them with respect to (c) density

(a) Calculate the density of NO₂ gas at 0.970 atm and 35 °C.

What is the density (in g/L) of hydrogen gas at 20.0 °C and a pressure of 1655 psi?

The density of a gas of unknown molar mass was measured as a function of pressure at 0 C, as in the table that follows. (b) Why is d>P not a constant as a function of pressure?

The density of a gas of unknown molar mass was measured as a function of pressure at 0 C, as in the table that follows. (a) Determine a precise molar mass for the gas. [Hint: Graph d>P versus P.]

An 11.5-mL sample of liquid butane (density = 0.573 g>mL) is evaporated in an otherwise empty container at a temperature of 28.5 °C. The pressure in the container following evaporation is 892 torr. What is the volume of the container?

What is the density of laughing gas, dinitrogen monoxide, N₂O, at a temperature of 325 K and a pressure of 113.0 kPa?

a gas with a molar mass of 26.54 g/mol is at a pressure of 172 torr and 27 °C. What is its density?

The density of a gas is 2.49 g/L at 3.00 atm and 25^oC. Calculate the molar mass of the gas.

What is the molar mass of an unknown gas with a density of 3.55 g/L at 2.00 atm and 55.0 °C?