1 mol N2 = 28g
30C = 303K
At STP, 1mol * 273K is proportional 24L * 760torr. (PV = nRT)
Then we do a little bit of stoichiometry...
10g * 1mol/28g * 24L*760torr/(1mol*273K) * 303K * xL/750torr = 9.6402 L
10.0g of N2 at 30C and 750torr should occupy 9.6402L
What volume is occupied by 20. 0 g of nitrogen (N2) gas at 30 degree C. and 800 mmHg?
0.004 gm/cm³
Convert all the pressures into one unit and then, using Dalton's Law of Partial Pressure, you just add all the pressures together. Using these conversions(101325Pa equals 1 ATM, 1 ATM equals 760 mmHg, 1 mmHg equals 1 torr), calculate each pressure into one unit(I used mmHg) 1013000 Pa nitrogen equals 7598 mmHg of nitrogen(make sure you round using sig figs) 700 mmHg of argon equals 700 mmHg of argon 1.20 ATM of helium equals 912 mmHg of helium 790 torr oxygen equals 790 mmHg of oxygen 0.50 ATM of carbon dioxide equals 380 mmHg of Carbon Dioxide Now add all the pressures and you get: 7598+700+912+790+380= 10380 mmHg If you need to have the answer in a particular unit: 10380 mmHg = 10380 torr = 13.66 ATM = 1384000 Pa = 1,384 kPa
Dalton says: "The partial pressure of a (non-condensing) gas in the mixture is proportional to its concentration." Since your total pressure is 1000 mmHg and the volumes all total to 1000 mL, you don't even need to take your shoes off to do the math.The nitrogen's volume is 780 ml of the total 1000 ml so its partial pressure is 780 mmHg of the total 1000 mmHg.
How To Calculate The Density Of Oxygen Gas ,O2, At 30 Deg. C And 700 MmHg
The volume ofhydrogen is 64,84 L.
800mm Hg Pressure and Volume are inversely proportional... thus is volume is halved (400ml -> 200ml) then pressure would double (400 mmHg -> 800 mmHg)
The volume is 0,446 L.
The volume of CO2 is 53,18 litres.
500. mmHg
747 mmHg
How do you calculate the density of oxygen gas (O2) at 30 degree C. and 700 mmHg?
Convert all the pressures into one unit and then, using Dalton's Law of Partial Pressure, you just add all the pressures together. Using these conversions(101325Pa equals 1 ATM, 1 ATM equals 760 mmHg, 1 mmHg equals 1 torr), calculate each pressure into one unit(I used mmHg) 1013000 Pa nitrogen equals 7598 mmHg of nitrogen(make sure you round using sig figs) 700 mmHg of argon equals 700 mmHg of argon 1.20 ATM of helium equals 912 mmHg of helium 790 torr oxygen equals 790 mmHg of oxygen 0.50 ATM of carbon dioxide equals 380 mmHg of Carbon Dioxide Now add all the pressures and you get: 7598+700+912+790+380= 10380 mmHg If you need to have the answer in a particular unit: 10380 mmHg = 10380 torr = 13.66 ATM = 1384000 Pa = 1,384 kPa
A fixed quantity of gas at a constant pressure exhibits a temperature of 27 degrees Celsius and occupies a volume of 10.0 L. Use Charles's law to calculate: the temperature of the gas in degrees Celsius in atmospheres if the volume is increased to 16.0 L
Dalton says: "The partial pressure of a (non-condensing) gas in the mixture is proportional to its concentration." Since your total pressure is 1000 mmHg and the volumes all total to 1000 mL, you don't even need to take your shoes off to do the math.The nitrogen's volume is 780 ml of the total 1000 ml so its partial pressure is 780 mmHg of the total 1000 mmHg.
How To Calculate The Density Of Oxygen Gas ,O2, At 30 Deg. C And 700 MmHg
2
The volume ofhydrogen is 64,84 L.
These three components are the three largest components of air. The total pressure of a gas mixture is just the sum of the partial pressures of each component. Air is a mixture and nitrogen, oxygen, and argon are the three biggest components. So, the atmospheric pressure (or air pressure) would be the sum of the partial pressure of each component of the air: Ptot=PPnitrogen + PPoxygen+ PPargon = 442 mmHg + 118.34 mmHg + 5.66 mmHg = 566 mmHg