Question
1.45 g of an unknown gas at 53 °C and 1.10 atm is stored in a 1.85-L flask.
What is the density of the gas
what is the molar mass of the gas
What is the density of the gas
what is the molar mass of the gas
Answers
DrBob222
The problem doesn't say the conditions you want for the density; i.e., is that density at 53 C and 1.10 atm or density at STP. I will assume you want it at STP. Therefore, we must correct the volume from 1.85 L to the volume at STP. So T goes from 326 K (273 + 53) to 273 K and pressure goes from 1.10 atm to 1.00 atm.
1.85 L x (273/326) x (1.10/1.00) = about 1.70 L but you should go through that yourself.
Then density = 1.45 g/1.70 = ?
Then density of a gas at STP = molar mass/22.4 L. You know density at STP, solve for molar mass.
1.85 L x (273/326) x (1.10/1.00) = about 1.70 L but you should go through that yourself.
Then density = 1.45 g/1.70 = ?
Then density of a gas at STP = molar mass/22.4 L. You know density at STP, solve for molar mass.