1) A sample of Xe gas has a volume of 852 mL, has a pressure of 523 mm Hg, and i
ID: 796767 • Letter: 1
Question
1) A sample of Xe gas has a volume of 852 mL, has a pressure of 523 mm Hg, and is at a temperature of 17.1 °C. Calculate the amount (in moles) of Xe in the gas sample. = ? mol
2) A sample of CCl4 with a pressure of 1.81 atm and a volume of 206 mL is allowed to react with excess CH4 at 195 °C.
Calculate the pressure of the CH2Cl2 produced in the reaction if it is transferred to a 1.61-L flask and cooled to 38 °C.
= ? atm
A sample of Xe gas has a volume of 852 mL, has a pressure of 523 mm Hg, and is at a temperature of 17.1 A degree C. Calculate the amount (in moles) of Xe in the gas sample = ? mol A sample of CCl4 with a pressure of 1.81 atm and a volume of 206 mL is allowed to react with excess CH4 at 195 A degree C Calculate the pressure of the CH2Cl2 produced in the reaction if it is transferred to a 1.61-L flask and cooled to 38 A degree C.Explanation / Answer
(1) Ideal gas equation: PV = nRT
Moles of Xe = n = PV/RT
= 523/760 x 825/1000/(0.08206 x (273.15 + 17.1))
= 0.0246 mol
(2) CH4 (g) + CCl4 (g) => 2 CH2Cl2 (g)
Ideal gas equation: PV = nRT
Moles of CCl4 = n = PV/RT
= 1.81 x 206/1000/(0.08206 x (273.15 + 195)) = 0.0097058 mol
Moles of CH2Cl2 = 2 x moles of CCl4
= 2 x 0.0097058 = 0.01941 mol
Pressure of CH2Cl2 = P = nRT/V
= 0.01941 x 0.08206 x (273.15 + 38)/1.61
= 0.308 atm
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