In: Chemistry
Inorganic Gasses Problems. Please only answer if you can answer it ALL and correctly:
4. A 1.21 g sample of ether was vaporized in a sealed 250 mL container at 50ºC. Pressure due to ether gas was 1173 torr. Determine molar mass of ether.
5. A 2 L container is charged with 2 atm of oxygen at 25ºC.
CH4(g) + 2 O2(g) ---> CO2(g) + 2 H2O(g)
Calculate the partial pressure of methane needed to react completely with the O2 in the vessel. What is the total pressure after the reaction is complete if the temperature has increased to 750ºC?
6. A mixture of oxygen and nitrogen is reacted with white phosphorus to remove all the oxygen from the mixture. The volume of the container decreases from 50 mL (when it contained both nitrogen and oxygen) to 35 mL (when only nitrogen is left) in order to keep the pressure inside the container unchanged. Calculate the partial pressure of oxygen in the original mixture if the total pressure in the original mixture was 740 torr.
4)
Assuming ether as a ideal gas
mass of ether =1.21 g
Volume =V= 250 mL = 0.250 L
Temperature = T = 50 + 273 = 323 K
Pressure = P =1173 torr
P=1.54 atm
Find the number of moles =
molar mass of ether = 83.16 g/mol
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5) CH4(g) + 2 O2(g) ---> CO2(g) + 2 H2O(g)
Partial pressure of O2 =P = 2 atm
Temperature = T= 25 + 273= 298 K
Volume = 2 L
Assuming O2 as ideal gas
Moles of O2 =
Moles of CH4 required =
Partial pressure of CH4 required = P =
Pressure of CH4 = 1 atm
If the reaction is completed at 25 deg C
Partial pressure exerted aby CO2 =
Partial pressure exerted by H2O gas =
Total pressure exerted by the gases = 2+1+1+2 = 6 atm pressure at 25 oC
Increased temperature = 750 + 273 = 1023 K
Pressure at 750 oC=
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6)
Total pressure of the mixture of gases (O2 + N2) = 740 torr
Volume of O2 present = 50-35 mL = 15 mL
Pressure of the mixture of 50 mL gases = 740 torr
Volume fraction of O2 = mole fraction of O2 =
Partial pressure of O2= mole fration x total pressure=