Imagine 6.32 g each of Ar, Kr, and He are placed in a 10.3 L fixed container at 27 ∘C. Calculate the partial pressure of each species. Calculate the total pressure of each species.

Partial pressure Ar = 0.378 atm

Partial pressure Kr = 0.180 atm

Partial pressure He = 3.776 atm

Total pressure = 4.334 atm

Explanation:

Step 1: Data given

Mass of Ar = 6.32 grams

Molar mass of Ar = 39.95 g/mol

Mass of Kr = 6.32 grams

Molar mass Kr = 83.80 g/mol

Mass of He = 6.32 g/mol

Molar mass of He = 4.00 g/mol

Volume = 10.3 L

Temperature = 27.0 °C

Step 2: Calculate moles

Moles = mass / molar mass

Moles Ar = 6.32 grams / 39.95 g/mol

Moles Ar = 0.158 moles

Moles Kr = 6.32 grams / 83.80 g/mol

Moles Kr = 0.0754 moles

Moles He = 6.32 grams / 4.00 g/mol

Moles He = 1.58 moles

Step 3: Calculate partial pressures

p*V= n*R*T

p(Ar) = (n*R*T)/V

⇒p(Ar) = the partial pressure of Ar gas = TO BE DETERMINED

⇒n= the number of moles of Ar =0.158 moles

⇒R = the gas constant = 0.08206 L*atm/mol*K

⇒T = the temperature = 27 +273 = 300 K

⇒V = the volume = 10.3 L

p(Ar) = (0.158 * 0.08206 * 300) / 10.3

p(Ar) = 0.378 atm

p(Kr) = (n*R*T)/V

⇒p(Kr) = the partial pressure of Kr gas = TO BE DETERMINED

⇒n= the number of moles of Kr =0.0754 moles

⇒R = the gas constant = 0.08206 L*atm/mol*K

⇒T = the temperature = 27 +273 = 300 K

⇒V = the volume = 10.3 L

p(Kr) = (0.0754 * 0.08206 * 300) / 10.3

p(Kr) = 0.180 atm

p(He) = (n*R*T)/V

⇒p(He) = the partial pressure of He gas = TO BE DETERMINED

⇒n= the number of moles of He =1.58 moles

⇒R = the gas constant = 0.08206 L*atm/mol*K

⇒T = the temperature = 27 +273 = 300 K

⇒V = the volume = 10.3 L

p(He) = (1.58 * 0.08206 * 300) / 10.3

p(He) = 3.776 atm

Step 4: Calculate the total pressure

Total pressure = p(Ar) +p(Kr) +p(He)

Total pressure = 0.378 atm + 0.180 atm + 3.776 atm

Total pressure = 4.334 atm

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