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Partial Pressure

Q. A mixture of 1.34 g H2 and 1.24 g He is placed in a 1.00-L container at 33°C. Calculate the partial pressure of each gas and the total pressure.

Solved • Oct 29, 2019

Partial Pressure

Q. A 5.00-L gas sample at 100.°C and 630. torr contains 44.8% neon and 55.2% argon by mass. What are the partial pressures of the individual gases?

Solved • Oct 29, 2019

Partial Pressure

Q. Refer to the diagram below. If the values were both opened and all three gases were allowed to diffuse and mix equally, what would the total pressure be? CO2 P = 2.13 V = 1.50 L H2 P = 0.861 atm V = 1.00 L Ar P = 1.15 atm V = 2.00 L

Solved • Oct 27, 2019

Partial Pressure

Q. A mixture carbon dioxide and carbon monoxide has a total pressure of 0.659 atm. If the carbon dioxide has a partial pressure that is twice that of carbon monoxide, determine the partial pressure of each gas in torr.

Solved • Oct 27, 2019

Partial Pressure

Q. Dichloromethane (CH2Cl2) and carbon tetrachloride (CCl4) have been listed as carcinogenic solvents by the FDA. What are the partical pressures of these substances in the vapor above a solution of 1.6 mol CH2Cl2 and 1.1 mol CCl4 at 23.5C. The vapor pressure of pure CH2Cl2 and CCl4 at 23.5C are 325 and 118 torr, respectively. Assume ideal behavior.

Solved • Oct 24, 2019

Partial Pressure

Q. A gaseous mixture contains 450.0 Torr H2(g), 383.3 Torr N2(g), and 68.7 Torr Ar(g). Calculate the mole fraction, 𝜒, of each of these gases. 𝜒H2= 𝜒N2= 𝜒Ar=

Solved • Oct 22, 2019

Partial Pressure

Q. A gas cylinder contains 1.55 mol He, 2.30 mol Ne, and 1.65 mol Ar. If the total pressure in the cylinder is 2510 mmHg, what is the partial pressure of each of the components? Assume constant temperature. 𝑃He= mmHg 𝑃Ne= mmHg 𝑃Ar=

Solved • Oct 22, 2019