H2O2 decomposes into water and oxygen...?

Question

A) Balance it, B) how many moles of O2 are produced and C)how many grams of H20 are formed.

If you could thoroughly explain how you got the answer I would appreciate it(have 19 more similar problems and a final on THursday[have everything else in chemistry downpacked]..I am completely lost)

Sorry, here's the needed information for part B

For Part B) 68g of H2O2 decompose, how many moles of O2 formed

Answer 1

H2O2 decomposes into H20(water) and O2(oxygen).The balanced equation is given below for u
2H2O2-------------2H2O+O2
From this equation we come to know that 2 moles of hydrogen peroxide(H2O2) decomposes into 2 moles of water and 1 mole of oxygen
Thus 68 gm of H202 is given
Now molecular weight of H202 is 2+(16)2=34
thus 68 gm consists of 2 moles which gives 1 mole of oxygen nothing but 32gm and 2 moles of water which is nothing but 36 gm

Answer 2

Start with the unbalaced equation: H2O2 -> H2O + O2. The only thing out of balance is the O2, so double the other terms to get 2H2O2 -> 2H2O + O2. Checking, we see that this is balanced.

The second part of the problem depends on the amount of either the reactant (H2O2) or of any of the results exist, and as stated none of this data is supplied so no definite answer can be given. If, for the sake of the example, we suppose that two moles of H2O2 are available (let's keep the math simple), then two moles of water and one mole of O2 are produced; the two moles of water weigh (obviously, I hope) 36 grams.

Answer 3

(A) Balance
Hydrogen peroxide decomposes into water and oxygen, according to the equation:

2H2O2 = 2H2O + O2
(68g) .....(36g)....(32g)

(B) Yield
The equation shows that 2 moles of hydrogen peroxide(68g) give 2 moles of water(36g) and one mole of oxygen