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?

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.

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