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[tex]\underline{\underline{\large{\green{\cal{✒GIVEN:}}}}}[/tex]
GIven the compounds H2O2, H2O and O2
[tex]\underline{\underline{\large{\green{\cal{REQUIRED:}}}}}[/tex]
Which is the balanced equation showing hydrogen peroxide (H2O2) decomposing into water (H2O) and oxygen (O2)?
[tex]\underline{\underline{\large{\green{\cal{SOLUTION:}}}}}[/tex]
Chemical equation is known to be balanced if the total moles of elements at the reactant is equal to the total moles at the product.
For the required decomposition of hydrogen peroxide:
1) Write the unbalanced equation:
[tex]\tt{H_{2}O_{2} \longrightarrow H_{2}O + O_{2}}[/tex]
2) Count the number of each type of atom on both sides of the equation:
On the reactant side (left):
• [tex]\tt{Hydrogen (H): \: 2}[/tex]
• [tex]\tt{Oxygen (O): \: 2}[/tex]
On the product side (right):
• [tex]\tt{Hydrogen \: (H): 2 \: (in H_{2}O)}[/tex]
• [tex]\tt{Oxygen \: (O): \: 1 \: (in H_{2}O) + 2 (in O_{2}) = 3}[/tex]
3) Balance the oxygen atoms first:
To balance the oxygen atoms, place a coefficient of 2 in front of H₂O₂ on the reactant side:
2 H₂O₂ → H₂O + O₂
Now count the atoms again:
On the reactant side (left):
• [tex]\tt{Hydrogen \: (H): \: 4}[/tex]
• [tex]\tt{Oxygen \: (O): \: 4}[/tex]
On the product side (right):
[tex]\tt{Hydrogen \: (H): \: 2 \: (in \: H_{2}O)}[/tex]
[tex]\tt{Oxygen (O): 1 (in H_{2}O) + 2 (in O_{2}) = 3}[/tex]
4) Balance the hydrogen atoms:
To balance the hydrogen atoms, place a coefficient of 2 in front of H₂O on the product side:
[tex]\tt{2 \: H_{2}O_{2} \longrightarrow 2 \: H_{2}O + O_{2}}[/tex]
Now count the atoms again:
On the reactant side (left):
• [tex]\tt{Hydrogen (H): \: 4}[/tex]
• [tex]\tt{Oxygen (O): \: 4}[/tex]
On the product side (right)
[tex]\tt{Hydrogen \: (H): \: 4 \: (in \: 2 \: H_{2}O)}[/tex]
[tex]\tt{Oxygen \: (O): \: 2 \: (in 2 H_{2}O) + 2 (in O_{2}) = 4}[/tex]
5) Verify that the equation is balanced:
Both sides have 4 hydrogen atoms and 4 oxygen atoms.
Therefore, the balanced equation is:
[tex]\tt{\purple{2 \: H_{2}O_{2} \longrightarrow 2 \: H_{2}O + O_{2}}}[/tex]
Hence, the balanced equation is [tex]\boxed{\large{\rm{\purple{2 \: H_{2}O_{2} \longrightarrow 2 \: H_{2}O + O_{2}}}}}[/tex]