Mm h2o2 = 34.02 g/mol mm h2o = 18.02 g/mol mm o2 = 32 g/mol 2h2o2 —> 2h2o + o2 if 14.3 moles of h2o2 is decomposed, how many grams of oxygen has are produced? show all your work to get full credit. ( ! )

  The grams   of oxygen that  are   produced  is  228.8 grams

  calculation

2H₂O₂ → 2H₂O +O₂

Step 1:  use  the  mole ratio to determine the moles of O₂

from equation above H₂O₂:O₂  is   2:1

therefore the  moles of O₂  = 14.3 moles ×1/2 = 7.15   moles

Step 2:  find  mass   of O₂

mass = moles ×  molar mass

= 7.15 moles × 32 g/mol =228.8 g

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: