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Find the constant, which i think is 3.7*10^-4 and multiply it by 1.0. and you should get your answer
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A tank contains N2 at 1.0 ATM and O2 at 2.0 ATM Helium is added to this tank until the total pressure is 6.0 ATM What is the partial pressure of the helium?
3.0 atm
A mixture of methane and helium is placed in a 2.0 l flask at 27 degrees the partial pressure of mathane is 0.72 ATM and the partial pressure of helium is 0.22 ATM What is the mole fraction of ch4?
0.77
The pressure of a sample of helium in a 1.00 L container is 0.988 ATM What is the new pressure if the sample is placed in a 4.40 L container?
The pressure of a sample of helium in a 1.00- L container is 0.988 atm. What is the new pressure if the sample is placed in a 200- L container
What is the pressure of 4 moles of helium in 50 L tank at 308 K?
2.02 atm
What is the pressure of 4 moles of helium in a 50 L tank at 308 K?
2.02 atm
A tank contains N2 at 1.0 ATM and O2 at 2.0 ATM Helium is added to this tank until the total pressure is 6.0 ATM What is the partial pressure of the helium?
3.0 atm
A pressurized tank contains a mixture of oxygen and helium If the partial pressure of oxygen is 10 atm and the partial pressure of helium is 32.8 atm what is the total pressure inside the tank?
42.8 atm fufurjthfhhudjd
Is the solubility of oxygen in blood at 2 ATM less than the same as or greater than at atmospheric pressure?
in my opinion, according to Henry's law - if pressure increase, solubility of gases will increase as well. I would say that the solubility of oxygen at 2 atm will be greater than at atm.
If the solubility of a gas in water in 4.0gL when the pressure of the gas above the water is 3.0 ATM what is the pressure of the gas above the water when solubility of the gas is 1.0?
.75
A mixture of methane and helium is placed in a 2.0 l flask at 27 degrees the partial pressure of mathane is 0.72 ATM and the partial pressure of helium is 0.22 ATM What is the mole fraction of ch4?
0.77
The pressure of a sample of helium in a 1.00 L container is 0.988 ATM What is the new pressure if the sample is placed in a 4.40 L container?
The pressure of a sample of helium in a 1.00- L container is 0.988 atm. What is the new pressure if the sample is placed in a 200- L container
What is the pressure of 4 moles of helium in 50 L tank at 308 K?
2.02 atm
What is the pressure of 4 moles of helium in a 50L tank at 308K Use PVnRT?
2.02 atm
What is the pressure of 4 moles of helium in a 50 L tank at 308 K?
2.02 atm
What is the molar mass of 18.12 g of gas exerting a pressure of 3.05 ATM on the walls of a 5.85 L container at 280 K?
The molar mass is 23,33 g.
How do you find out the molar mass of a gas given density temperature and pressure?
MolarMass = [density x gas constant x temperature(in kelvin)] / pressure (in atm)
What is the total pressure in ATM of 10.13 kpa nitrogen 720 mm argon 1.25 ATM of helium 780 torr oxygen and 0.92 carbon dioxide?
At first recalculate mmHg and torr to atm. Then you add them (3 values in atm.) up to get total pressure.
