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Sagot :
To balance the chemical equation [tex]\( \text{H}_2\text{O} \rightarrow \text{H}_2 + \text{O}_2 \)[/tex], we need to determine the coefficients for [tex]\( \text{H}_2\text{O} \)[/tex], [tex]\( \text{H}_2 \)[/tex], and [tex]\( \text{O}_2 \)[/tex] that will ensure the same number of each type of atom on both sides of the equation.
1. Identify the reactants and products:
The reactant is [tex]\( \text{H}_2\text{O} \)[/tex] (water), and the products are [tex]\( \text{H}_2 \)[/tex] (hydrogen gas) and [tex]\( \text{O}_2 \)[/tex] (oxygen gas).
2. Count the number of each type of atom on both sides of the equation:
- On the left side (reactants):
- Hydrogen (H): 2 atoms (from [tex]\( \text{H}_2\text{O} \)[/tex])
- Oxygen (O): 1 atom (from [tex]\( \text{H}_2\text{O} \)[/tex])
- On the right side (products):
- Hydrogen (H): 2 atoms (from [tex]\( \text{H}_2 \)[/tex])
- Oxygen (O): 2 atoms (from [tex]\( \text{O}_2 \)[/tex])
3. Determine the coefficients that balance the equation:
Upon analyzing the balanced equation, we see that we need to adjust the coefficients so that the number of hydrogen and oxygen atoms on both sides are equal. The balanced equation should look like:
[tex]\[ 2\text{H}_2\text{O} \rightarrow 2\text{H}_2 + \text{O}_2 \][/tex]
Here's the breakdown:
- For hydrogen: [tex]\( 2 \)[/tex] molecules of [tex]\( \text{H}_2\text{O} \)[/tex] (each having 2 hydrogen atoms) will give [tex]\( 4 \)[/tex] hydrogen atoms in total, which corresponds to [tex]\( 2 \)[/tex] molecules of [tex]\( \text{H}_2 \)[/tex] (each having 2 hydrogen atoms).
- For oxygen: [tex]\( 2 \)[/tex] molecules of [tex]\( \text{H}_2\text{O} \)[/tex] (each having 1 oxygen atom) will give [tex]\( 2 \)[/tex] oxygen atoms in total, which corresponds exactly to [tex]\( 1 \)[/tex] molecule of [tex]\( \text{O}_2 \)[/tex] (having 2 oxygen atoms).
In conclusion, the balanced equation is:
[tex]\[ 2\text{H}_2\text{O} \rightarrow 2\text{H}_2 + \text{O}_2 \][/tex]
Thus, the coefficients that balance the equation are 2 for [tex]\( \text{H}_2\text{O} \)[/tex], 2 for [tex]\( \text{H}_2 \)[/tex], and 1 for [tex]\( \text{O}_2 \)[/tex].
- Coefficient for [tex]\( \text{H}_2\text{O} \)[/tex] is 2.
- Coefficient for [tex]\( \text{H}_2 \)[/tex] is 2.
- Coefficient for [tex]\( \text{O}_2 \)[/tex] is 1.
So, using the dropdown menu to select the coefficients:
- For [tex]\( \text{H}_2\text{O} \)[/tex]: 2
- For [tex]\( \text{H}_2 \)[/tex]: 2
- For [tex]\( \text{O}_2 \)[/tex]: 1
1. Identify the reactants and products:
The reactant is [tex]\( \text{H}_2\text{O} \)[/tex] (water), and the products are [tex]\( \text{H}_2 \)[/tex] (hydrogen gas) and [tex]\( \text{O}_2 \)[/tex] (oxygen gas).
2. Count the number of each type of atom on both sides of the equation:
- On the left side (reactants):
- Hydrogen (H): 2 atoms (from [tex]\( \text{H}_2\text{O} \)[/tex])
- Oxygen (O): 1 atom (from [tex]\( \text{H}_2\text{O} \)[/tex])
- On the right side (products):
- Hydrogen (H): 2 atoms (from [tex]\( \text{H}_2 \)[/tex])
- Oxygen (O): 2 atoms (from [tex]\( \text{O}_2 \)[/tex])
3. Determine the coefficients that balance the equation:
Upon analyzing the balanced equation, we see that we need to adjust the coefficients so that the number of hydrogen and oxygen atoms on both sides are equal. The balanced equation should look like:
[tex]\[ 2\text{H}_2\text{O} \rightarrow 2\text{H}_2 + \text{O}_2 \][/tex]
Here's the breakdown:
- For hydrogen: [tex]\( 2 \)[/tex] molecules of [tex]\( \text{H}_2\text{O} \)[/tex] (each having 2 hydrogen atoms) will give [tex]\( 4 \)[/tex] hydrogen atoms in total, which corresponds to [tex]\( 2 \)[/tex] molecules of [tex]\( \text{H}_2 \)[/tex] (each having 2 hydrogen atoms).
- For oxygen: [tex]\( 2 \)[/tex] molecules of [tex]\( \text{H}_2\text{O} \)[/tex] (each having 1 oxygen atom) will give [tex]\( 2 \)[/tex] oxygen atoms in total, which corresponds exactly to [tex]\( 1 \)[/tex] molecule of [tex]\( \text{O}_2 \)[/tex] (having 2 oxygen atoms).
In conclusion, the balanced equation is:
[tex]\[ 2\text{H}_2\text{O} \rightarrow 2\text{H}_2 + \text{O}_2 \][/tex]
Thus, the coefficients that balance the equation are 2 for [tex]\( \text{H}_2\text{O} \)[/tex], 2 for [tex]\( \text{H}_2 \)[/tex], and 1 for [tex]\( \text{O}_2 \)[/tex].
- Coefficient for [tex]\( \text{H}_2\text{O} \)[/tex] is 2.
- Coefficient for [tex]\( \text{H}_2 \)[/tex] is 2.
- Coefficient for [tex]\( \text{O}_2 \)[/tex] is 1.
So, using the dropdown menu to select the coefficients:
- For [tex]\( \text{H}_2\text{O} \)[/tex]: 2
- For [tex]\( \text{H}_2 \)[/tex]: 2
- For [tex]\( \text{O}_2 \)[/tex]: 1
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