When 90 g of water is split by electrolysis (2h2o → 2h2 +o2) at stp, how many liters of oxygen gas will be collected? question 6 options: 44.8 l 22.4 l 56.0 l 67.2 l

If the molecular weight of water is 18g/mol, then the number of water molecule would be: 90g/ (18g/mol)= 5 moles.

In the reaction equation, 2 H2O molecules will result in 1 O2 molecule. Then, the amount of O2 formed would be: 5 moles * (1/2)= 2.5 moles.

In STP, an ideal gas will have 22.4 liters of volume per mol. Then, the volume of the oxygen formed would be: 2.5 moles * (22.4l/mol)= 56.0 L 

What are the statements?