Question

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help me with the question attached.
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Answer 1

Answer:

$\fbox {(2) 4.9}$

Explanation:

Applying the Ideal Gas Equation :

$\boxed {PV = nRT}$

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.

Answer 2

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