Open Question
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?
7. Gases
The Ideal Gas Law: Density
Back7. Gases
The Ideal Gas Law: Density
- Multiple Choice
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.
- Multiple Choice
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?
- Multiple ChoiceCalculate the density of argon gas at 22.5℃ and a pressure of 2.0 atm.
- Open Question
What is the density of laughing gas, dinitrogen monoxide, N2O, at a temperature of 325 K and a pressure of 113.0 kPa?
- Open Question
The density of a gas is 2.49 g/L at 3.00 atm and 25oC. Calculate the molar mass of the gas.
- Open Question
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?
- Multiple ChoiceAt what temperature in Kelvin does sulfur hexafluoride (SF6) have a density of 0.5550 g/L at a pressure of 0.8210 atm?
- Multiple ChoiceUsing 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)
- Multiple ChoiceUsing the Ideal Gas Law, calculate the density of CO2 gas in g/L at 27°C and 0.50 atm pressure.
- Multiple ChoiceWhat 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?
- Multiple ChoiceWhat 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?
- Multiple ChoiceWhat is the density of hydrogen sulfide (H₂S) at 1.7 atm and 265 K? Answer in units of g/L.
- Multiple ChoiceWhat is the density of nitrogen gas (N₂) at 67.3°C and 0.288 atm, assuming ideal gas behavior?
- Multiple ChoiceWhat is the density of sulfur trioxide gas (SO3) at 315 K and 2.10 atm, given that the molar mass of SO3 is 80.07 g/mol?