How many grams of water do you have to decompose if you want to prepare 34.7 g of oxygen?

Try this solution:

The equation of the reaction is:

2H₂O⇒2H₂↑+O₂↑ where m(O₂)=34.7gr.

M(O₂)=16*2=32 (gr./mol);

ν(O₂)=m(O₂)/M(O₂)=34.7/32=1.084375 (mol).

According to the equation of the reaction ν(H₂O)=2ν(O₂)=2*1.084375=2.16875 (mol);

M(H₂O)=2+16=18 (gr./mol).

m(H₂O)=M(H₂O)*ν(H₂O)=18*2.16875=39.0375 gr.

39.0375 gr.

i just got this problem. it's 90.3

the dependant variable is spilled water

the independent is the heat