Question

1- A mixture of hydrogen and argon gases, in a 8.69 L flask at 77 °C, contains 0.477 grams of hydrogen and 7.10 grams of argon. The partial pressure of argon in the flask is ____ atm and the total pressure in the flask is ____ atm.

2- A mixture of methane and carbon dioxide gases is maintained in a 7.86 L flask at a pressure of 1.93 atm and a temperature of 39 °C. If the gas mixture contains 5.65 grams of methane, the number of grams of carbon dioxide in the mixture is ____ g.

3- The stopcock connecting a 2.65 L bulb containing oxygen gas at a pressure of 8.75 atm, and a 5.41 L bulb containing carbon dioxide gas at a pressure of 2.80 atm, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is ____ atm.

4- A mixture of helium and carbon dioxide gases contains helium at a partial pressure of 205 mm Hg and carbon dioxide at a partial pressure of 760 mm Hg. What is the mole fraction of each gas in the mixture?

X_He =
X_CO2 =

5- A mixture of nitrogen and methane gases at a total pressure of 694 mm Hg contains nitrogen at a partial pressure of 517 mm Hg. If the gas mixture contains 7.04 grams of nitrogen, how many grams of methane are present?

____ g CH₄

Answer 1

hole of H = 0.47-0.9385 mall q mole of Ar= = 0.174 mole 7.10 39.948 total mole=0.4155 mole Prosal (total poussere] = nx RXT = 0.41557.082x350 8.69 = 1.372 atm partial pressure of Ar= 0.177 x 1.372 atm 0.4155 0.584 atm = ☺ total moles = PxV, 1.93 x 7.86 -0.5929 RXT :082 x 312 moles of Cha = 5.65 = 0.353 mole of Co, = 0.5929 -0.353=0.239 gm of co = 10.516 gm

Total moles mole of O, + mole of Co, 9:15*2.65 + 2.8075.41 - RXT RXT Princex (2:6545.41 RXT Prince = 4.456 atm Ptotal = pre + bco, = 205 + 760 Protal = 965 - Xhe = me 205 = 0.212 965 - 760 = 0-787 965 moll of N = 7.04 - 0.2514 mole 28 mole of Ng 517 694 - 0.2514 0.2514+ mol mole of N t molest of cha

mea of Cr, - 0.086 069 gm of CHg = mole x molar mass = 0.086069 x16 = 1.377 gm