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.

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

,

where

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?

answer: cellular respiration takes in food and uses it to create atp, a chemical which the cell uses for energy. usually, this process uses oxygen, and is called aerobic respiration. it has four stages known as glycolysis, link reaction, the krebs cycle, and the electron transport chain.