What is the mass present in a 10.0l container of oxygen at a pressure of 105kpa and 20 degrees celsius

1.31 × 10⁴ grams.

Explanation

Assume that oxygen acts like an ideal gas. In other words, assume that the oxygen here satisfies the ideal gas law:

,

where

the pressure on the gas, ; the volume of the gas, ; the number of moles of the gas, which needs to be found; the absolute temperature of the gas, . the ideal gas constant, if P, V, and T are in their corresponding SI units: Pa, m³, and K.

Apply the ideal gas law to find :

.

In other words, there are 410.3 moles of O₂ molecules in that container.

There are two oxygen atoms in each O₂ molecules. The mass of mole of O₂ molecules will be . The mass of 410.3 moles of O₂ will be:

.

What would be the mass of oxygen in the container if the pressure is approximately the same as STP at or   instead?

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