Question

A sample of oxygen, o2, occupies a volume of 0. 65 l at 11°c under 0. 50 atm of pressure. (r = 0. 08205 latm/molk). how many moles of o2 are present in this sample? (pv = nrt) group of answer choices

Answer 1

It is calculated that 0.014 moles of oxygen (O₂) are present in the given sample by using the ideal gas law.

Calculation:

Provided that :

Temperature, T = 273+11 K = 284 K

Pressure, P = 0.5 atm

Volume, V = 0.65 L

Ideal gas constant,R = 0.08205 L atm/mol K

According to the ideal gas law,

we know the formula, PV = nRT

or, n = PV / RT = (0.5 * 0.65) / (0.08205 * 284)

or, n = 0.0139 ≈ 0.014 mole

What is the ideal gas law?

• The universal gas equation, often known as the ideal gas law, is the formula of state for a fictitious ideal gas. Although it has several restrictions, it is a decent approximation of the behavior of numerous gases under various circumstances.
• Benoît Paul Émile Clapeyron introduced it for the first time in 1834 as a synthesis of the experimental Boyle's law, Charles' law, Avogadro's law, and Gay-Lussac's law.

Learn more about ideal gas law here:

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