To form 100 g of #H_2O_2#, 5.927 g of H must react with 94.073 g of O. How many grams of O would be needed to form 104 g of #H_2O_2#?

1 Answer
Jun 14, 2018

Answer:

Well, what is #5.927%# of #104*g#?

Explanation:

And I make this....

#5.927%xx104*g=6.164*g#

And let us just check this...and examine the empirical formula of the #104*g# mass...and for this we divide thru by the ATOMIC mass of each constituent element...

#"Moles of hydrogen"=(6.164*g)/(1.00794*g*mol^-1)=6.116*mol#

#"Moles of oxygen"=(104*g-6.164*g)/(16.00*g*mol^-1)=6.116*mol#

And thus the empirical formula is simply #HO#...why is this different from the chemical formula of hydrogen peroxide?