The correct statement that explains why the equation \( \text{H}_2\text{O}_2 \rightarrow 2\text{H}_2\text{O} + \text{O}_2 \) is not balanced is:
Two H2O2 molecules should decompose to form the given products.
Here's why:
Looking at the unbalanced equation:
- On the left side (reactants), there is 1 molecule of \( \text{H}_2\text{O}_2 \).
- On the right side (products), there are 2 molecules of \( \text{H}_2\text{O} \) and 1 molecule of \( \text{O}_2 \).
Now let's count the number of each type of atom:
-
Hydrogen (H):
- Reactants: 2 (from \( \text{H}_2\text{O}_2 \))
- Products: 4 (2 from each of the 2 water molecules)
-
Oxygen (O):
- Reactants: 2 (from \( \text{H}_2\text{O}_2 \))
- Products: 3 (2 from the two water molecules and 1 from the oxygen gas)
Since there are 4 hydrogen atoms and 3 oxygen atoms in the products, while we started with only 2 hydrogen and 2 oxygen atoms from 1 \( \text{H}_2\text{O}_2 \), the equation is not balanced. To balance it correctly, you would indeed require 2 molecules of \( \text{H}_2\text{O}_2 \) to properly yield the products.