Step 1
Oxygen gas is assumed to be an ideal gas, so it is applied:
[tex]p\text{ x V = n x R x T}[/tex]
p = pressure
V = volume
n = number of moles
R = gas constant
T = absolute temperature
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Step 2
Information provided:
V = unknown
p = 1.00 atm
n = 2.00 moles
T = 273 K
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Information needed:
R = 0.082 atm L/mol K
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Step 3
From step 1, V is found as follows:
[tex]\begin{gathered} p\text{ x V = n x R x T} \\ V\text{ = }\frac{n\text{ x R x T}}{p} \\ V\text{ = }\frac{2.00\text{ moles x 0.082 }\frac{atm\text{ L}}{mol\text{ K}}\text{ x 273 K}}{1.00\text{ atm }} \\ V\text{ = 44.77 L = 44.8 L \lparen apporox.\rparen} \end{gathered}[/tex]
Answer: 44.8 L
