Respuesta :

Answer:

[tex]\fbox {(2) 4.9}[/tex]

Explanation:

Applying the Ideal Gas Equation :

[tex]\boxed {PV = nRT}[/tex]

Finding n :

  • n = 64 g / 32 g/mole (Oxygen is diatomic)
  • n = 2 moles

Solving for P :

  • P = 2 × 0.0831 × 300 / 10 (Temp. should be converted to K)
  • P = 60 × 0.0831
  • P = 4.9

∴ The pressure inside the flask in bar is 4.9.

Moles of oxygen

  • Given mass/Molar mass
  • 64g/32g/mol
  • 2mol

Temperature=273+27=300K

Apply ideal gas equation

  • PV=nRT
  • P=nRT/V
  • P=2(0.0831)(300)/10
  • P=4.9bar

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