Question

Hydrogen peroxide, H2O2 decomposed to formed water and oxygen.

2H2O2 -> 2H2O + O2

If 1.7 g of hydrogen peroxide decomposes, calculate:
(i) the volume of oxygen produced at room condition.
(ii)the number of molecules of oxygen produced​

Answer 1

Answer:

Explanation:

Your equation is not correctly balanced. The correct equation is as follows:

2H2O2→2H2O+O2

First, calculate the moles of H2O2 reacting. In order to do this, we must evaluate the relative molecular mass (Mr) of hydrogen peroxide:

Mr (H2O2) =2×1+2×16=34

mol=mMr=6834=2 moles

Next, we must compare the moles of hydrogen peroxide and oxygen gas. According to the corrected equation, this mole ratio is as shown below:

mol (H2O2) : mol (O2)

2 : 1

Thus, the moles of oxygen produced in this reaction will be exactly half the moles of hydrogen peroxide reacting.

∴ mol (O2)=mol(H2O2)2=22=1 mole

Finally, convert from moles into mass, given that Mr (O2)=32 :

mol=mMr⇒m=mol×M