1. A cylinder contains 3.00 mol of Ar, 6.00 mol of Ne, and 1.00 mol of He. At 200 K, the total pressure is found to be 3.00 a What is the partial pressure of Ne gas in the cylinder? 01.80 atm 00.900 atm 02.00 atm 01.00 atm 18.0 atm

A sample contains 10.5 g N2 (MW = 28.02 g/mol), 6.5 g He (MW = 4.00 g/mol), and 34.6 g CO2 (MW = 44.01 g/mol). If this sample has a total pressure of 15.0 atm, calculate the partial pressure due to the He (PHe)Select one:12.3 atm 8.7 atm 5.0 atm 3.5 atm

A gaseous mixture contains 12.4 g of N2 and 12.4 g of 02 that exerts a total pressure of 1.23 atm. What will the be the partial pressure of N2 in the mixture? 0.615 atm O 0.656 atm O 0.375 atm O 0.885 atm

A 5.00-mol sample of oxygen gas is confined to a pressure of 5 atm at a temperature of 27 degrees Celsius. What must be the volume of the vessel containing these oxygen gas molecules? (*Solution required)   a. 2494.2 m³ b. 0.02 m³ c. 12.47 x 10³ m³ d. 0.12 m³

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gas mixture consists of H2, SO2, and N2. The partial pressures of each gas are: H2 = 0.15 atm, SO2 = 1.50 atm, N2= 3.30 atm. The pressure of the mixture is: a) 4.95 atm b) 11.4 atm c) 1 atm d) 10 atm

A sample contains 2.0 moles of He gas and 6.0 moles of Ar gas. What is the mole fraction of He gas (XHe)? 0.33 0.75 0.25 2.0

A sealed 2.0L container at 380 K is filled with 0.75 g of hydrogen gas and 3.25 g of oxygen gas and combusted to produce water vapor. what is the partial pressure of hydrogen gas after combustion if the temperature is maintained at 380 K there is no hydrogen gas left over since oxygen gas is the limiting reactant  2.63 atm H2 4.55 atm H2  5.80 atm H2 none of the above