Westonci.ca is the premier destination for reliable answers to your questions, brought to you by a community of experts. Experience the convenience of getting reliable answers to your questions from a vast network of knowledgeable experts. Connect with a community of professionals ready to provide precise solutions to your questions quickly and accurately.
Sagot :
To balance the combustion reaction of octane, [tex]\( C_8H_{18} \)[/tex], with oxygen, [tex]\( O_2 \)[/tex], into carbon dioxide, [tex]\( CO_2 \)[/tex], and water, [tex]\( H_2O \)[/tex], we need to ensure that we have the same number of each type of atom on both sides of the equation. Here is the step-by-step process to balance the equation:
1. Write the unbalanced equation:
[tex]\[ C_8H_{18} + O_2 \rightarrow \_ CO_2 + \_ H_2O \][/tex]
2. Balance the number of carbon (C) atoms:
- There are 8 carbon atoms in [tex]\( C_8H_{18} \)[/tex].
- We need 8 carbon atoms in the products, which will be in the form of [tex]\( CO_2 \)[/tex].
- Therefore, the coefficient for [tex]\( CO_2 \)[/tex] will be 8:
[tex]\[ C_8H_{18} + O_2 \rightarrow 8 CO_2 + \_ H_2O \][/tex]
3. Balance the number of hydrogen (H) atoms:
- There are 18 hydrogen atoms in [tex]\( C_8H_{18} \)[/tex].
- Water ([tex]\( H_2O \)[/tex]) contains 2 hydrogen atoms per molecule.
- To balance 18 hydrogen atoms, we need [tex]\( \frac{18}{2} = 9 \)[/tex] water molecules:
[tex]\[ C_8H_{18} + O_2 \rightarrow 8 CO_2 + 9 H_2O \][/tex]
4. Balance the number of oxygen (O) atoms:
- On the right-hand side, we have:
- [tex]\( 8 CO_2 \)[/tex] molecules, each providing 2 oxygen atoms, totaling [tex]\( 8 \times 2 = 16 \)[/tex] oxygen atoms.
- [tex]\( 9 H_2O \)[/tex] molecules, each providing 1 oxygen atom, totaling 9 oxygen atoms.
- Therefore, the total number of oxygen atoms on the right-hand side is [tex]\( 16 + 9 = 25 \)[/tex].
- Oxygen ([tex]\( O_2 \)[/tex]) contains 2 oxygen atoms per molecule.
- To balance 25 oxygen atoms, we need [tex]\( \frac{25}{2} = 12.5 \)[/tex] oxygen molecules:
[tex]\[ C_8H_{18} + 12.5 O_2 \rightarrow 8 CO_2 + 9 H_2O \][/tex]
5. Avoid fractions by multiplying the entire equation by 2:
- This will give us whole numbers for all coefficients:
[tex]\[ 2 C_8H_{18} + 25 O_2 \rightarrow 16 CO_2 + 18 H_2O \][/tex]
Thus, the balanced combustion reaction for octane, [tex]\( C_8H_{18} \)[/tex], is:
[tex]\[ 2 C_8H_{18} + 25 O_2 \rightarrow 16 CO_2 + 18 H_2O \][/tex]
In this balanced equation, the coefficients are:
- [tex]\( C_8H_{18} \)[/tex]: 2
- [tex]\( O_2 \)[/tex]: 25
- [tex]\( CO_2 \)[/tex]: 16
- [tex]\( H_2O \)[/tex]: 18
So, the coefficients for the balanced equation are:
[tex]\[ [2, 25, 16, 18] \][/tex]
1. Write the unbalanced equation:
[tex]\[ C_8H_{18} + O_2 \rightarrow \_ CO_2 + \_ H_2O \][/tex]
2. Balance the number of carbon (C) atoms:
- There are 8 carbon atoms in [tex]\( C_8H_{18} \)[/tex].
- We need 8 carbon atoms in the products, which will be in the form of [tex]\( CO_2 \)[/tex].
- Therefore, the coefficient for [tex]\( CO_2 \)[/tex] will be 8:
[tex]\[ C_8H_{18} + O_2 \rightarrow 8 CO_2 + \_ H_2O \][/tex]
3. Balance the number of hydrogen (H) atoms:
- There are 18 hydrogen atoms in [tex]\( C_8H_{18} \)[/tex].
- Water ([tex]\( H_2O \)[/tex]) contains 2 hydrogen atoms per molecule.
- To balance 18 hydrogen atoms, we need [tex]\( \frac{18}{2} = 9 \)[/tex] water molecules:
[tex]\[ C_8H_{18} + O_2 \rightarrow 8 CO_2 + 9 H_2O \][/tex]
4. Balance the number of oxygen (O) atoms:
- On the right-hand side, we have:
- [tex]\( 8 CO_2 \)[/tex] molecules, each providing 2 oxygen atoms, totaling [tex]\( 8 \times 2 = 16 \)[/tex] oxygen atoms.
- [tex]\( 9 H_2O \)[/tex] molecules, each providing 1 oxygen atom, totaling 9 oxygen atoms.
- Therefore, the total number of oxygen atoms on the right-hand side is [tex]\( 16 + 9 = 25 \)[/tex].
- Oxygen ([tex]\( O_2 \)[/tex]) contains 2 oxygen atoms per molecule.
- To balance 25 oxygen atoms, we need [tex]\( \frac{25}{2} = 12.5 \)[/tex] oxygen molecules:
[tex]\[ C_8H_{18} + 12.5 O_2 \rightarrow 8 CO_2 + 9 H_2O \][/tex]
5. Avoid fractions by multiplying the entire equation by 2:
- This will give us whole numbers for all coefficients:
[tex]\[ 2 C_8H_{18} + 25 O_2 \rightarrow 16 CO_2 + 18 H_2O \][/tex]
Thus, the balanced combustion reaction for octane, [tex]\( C_8H_{18} \)[/tex], is:
[tex]\[ 2 C_8H_{18} + 25 O_2 \rightarrow 16 CO_2 + 18 H_2O \][/tex]
In this balanced equation, the coefficients are:
- [tex]\( C_8H_{18} \)[/tex]: 2
- [tex]\( O_2 \)[/tex]: 25
- [tex]\( CO_2 \)[/tex]: 16
- [tex]\( H_2O \)[/tex]: 18
So, the coefficients for the balanced equation are:
[tex]\[ [2, 25, 16, 18] \][/tex]
Thank you for trusting us with your questions. We're here to help you find accurate answers quickly and efficiently. We appreciate your time. Please revisit us for more reliable answers to any questions you may have. We're glad you chose Westonci.ca. Revisit us for updated answers from our knowledgeable team.