Oxygen gas is commonly sold in 46.5 L steel containers at a pressure of 130 atm.?

Oxygen gas is commonly sold in 46.5 L steel containers at a pressure of 130 atm.
What volume (in liters) would the gas occupy at a pressure of 1.03 atm if its temperature remained unchanged?

Initial : P₁ = 130 atm, V₁ = 46.5 L
Final : P₂ = 1.03 atm, V₂ = ? L

For a fixed amount of gas at constant temperature, P₁V₁ = P₂V₂
Then, V₂ = V₁ × (P₁/P₂)

Final pressure, V₂ = (46.5 L) × (130/1.03) = 5870 L


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What volume (in liters) would the gas occupy if its temperature was raised from 21.0 °C to 35.5 °C at constant 130 atm ?

Initial : V₁ = 46.5 L, T₁ = (273.2 + 21.0) K = 294.2 K
Final : V₂ = ? L, T₂ = (273.2 + 35.5) K = 308.7 K

For a fixed amount of gas at constant pressure, V₁/T₁ = V₂/T₂
Then, V₂ = V₁ × (T₂/T₁)

Final volume, V₂ = (46.5 L) × (308.7/294.2) = 48.8 L

Ok