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.

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i  

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