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Certainly! To determine the correct chemical equation for the burning of propane ([tex]\(C_3H_8\)[/tex]), we need to identify which one matches the balanced combustion reaction of propane in the gas phase. The general form for the combustion of a hydrocarbon [tex]\(C_xH_y\)[/tex] in the presence of oxygen [tex]\(O_2\)[/tex] is:
[tex]\[ C_xH_y + O_2 \rightarrow CO_2 + H_2O \][/tex]
For propane, [tex]\(C_3H_8\)[/tex]:
[tex]\[ C_3H_8 + O_2 \rightarrow CO_2 + H_2O \][/tex]
Next, we balance the chemical equation to ensure we have the same number of each type of atom on both sides of the equation.
### Step-by-Step Balancing:
1. Write down the unbalanced equation:
[tex]\[ C_3H_8 + O_2 \rightarrow CO_2 + H_2O \][/tex]
2. Balance carbon (C) atoms:
- There are 3 carbon atoms in [tex]\(C_3H_8\)[/tex].
- On the product side, each [tex]\(CO_2\)[/tex] molecule has 1 carbon atom.
- Therefore, we need 3 [tex]\(CO_2\)[/tex] molecules to balance the carbon atoms.
[tex]\[ C_3H_8 + O_2 \rightarrow 3 CO_2 + H_2O \][/tex]
3. Balance hydrogen (H) atoms:
- There are 8 hydrogen atoms in [tex]\(C_3H_8\)[/tex].
- On the product side, each [tex]\(H_2O\)[/tex] molecule has 2 hydrogen atoms.
- Therefore, we need 4 [tex]\(H_2O\)[/tex] molecules to balance the hydrogen atoms.
[tex]\[ C_3H_8 + O_2 \rightarrow 3 CO_2 + 4 H_2O \][/tex]
4. Balance oxygen (O) atoms:
- On the product side, we now have:
- 3 [tex]\(CO_2\)[/tex] molecules, each contributing 2 oxygen atoms for a total of [tex]\(3 \times 2 = 6\)[/tex] oxygen atoms.
- 4 [tex]\(H_2O\)[/tex] molecules, each contributing 1 oxygen atom for a total of [tex]\(4 \times 1 = 4\)[/tex] oxygen atoms.
- Therefore, we need [tex]\(6 + 4 = 10\)[/tex] oxygen atoms in total.
- On the reactant side, [tex]\(O_2\)[/tex] is a diatomic molecule, so each [tex]\(O_2\)[/tex] contributes 2 oxygen atoms.
- To balance, we need [tex]\(10 \div 2 = 5\)[/tex] [tex]\(O_2\)[/tex] molecules.
[tex]\[ C_3H_8 + 5 O_2 \rightarrow 3 CO_2 + 4 H_2O \][/tex]
### Verification:
1. Count each type of atom on both sides of the equation:
- Reactants: [tex]\(C_3H_8 + 5 O_2\)[/tex]
- Carbon: 3
- Hydrogen: 8
- Oxygen: [tex]\(5 \times 2 = 10\)[/tex]
- Products: [tex]\(3 CO_2 + 4 H_2O\)[/tex]
- Carbon: 3
- Hydrogen: 8
- Oxygen: [tex]\(3 \times 2 + 4 \times 1 = 6 + 4 = 10\)[/tex]
All atoms balance correctly on both sides of the equation, verifying the equation is correct.
### Conclusion:
The balanced chemical equation for the burning of propane where all reactants and products are in the gas phase is:
[tex]\[ \boxed{C_3H_8(g) + 5 O_2(g) \rightarrow 3 CO_2(g) + 4 H_2O(g)} \][/tex]
[tex]\[ C_xH_y + O_2 \rightarrow CO_2 + H_2O \][/tex]
For propane, [tex]\(C_3H_8\)[/tex]:
[tex]\[ C_3H_8 + O_2 \rightarrow CO_2 + H_2O \][/tex]
Next, we balance the chemical equation to ensure we have the same number of each type of atom on both sides of the equation.
### Step-by-Step Balancing:
1. Write down the unbalanced equation:
[tex]\[ C_3H_8 + O_2 \rightarrow CO_2 + H_2O \][/tex]
2. Balance carbon (C) atoms:
- There are 3 carbon atoms in [tex]\(C_3H_8\)[/tex].
- On the product side, each [tex]\(CO_2\)[/tex] molecule has 1 carbon atom.
- Therefore, we need 3 [tex]\(CO_2\)[/tex] molecules to balance the carbon atoms.
[tex]\[ C_3H_8 + O_2 \rightarrow 3 CO_2 + H_2O \][/tex]
3. Balance hydrogen (H) atoms:
- There are 8 hydrogen atoms in [tex]\(C_3H_8\)[/tex].
- On the product side, each [tex]\(H_2O\)[/tex] molecule has 2 hydrogen atoms.
- Therefore, we need 4 [tex]\(H_2O\)[/tex] molecules to balance the hydrogen atoms.
[tex]\[ C_3H_8 + O_2 \rightarrow 3 CO_2 + 4 H_2O \][/tex]
4. Balance oxygen (O) atoms:
- On the product side, we now have:
- 3 [tex]\(CO_2\)[/tex] molecules, each contributing 2 oxygen atoms for a total of [tex]\(3 \times 2 = 6\)[/tex] oxygen atoms.
- 4 [tex]\(H_2O\)[/tex] molecules, each contributing 1 oxygen atom for a total of [tex]\(4 \times 1 = 4\)[/tex] oxygen atoms.
- Therefore, we need [tex]\(6 + 4 = 10\)[/tex] oxygen atoms in total.
- On the reactant side, [tex]\(O_2\)[/tex] is a diatomic molecule, so each [tex]\(O_2\)[/tex] contributes 2 oxygen atoms.
- To balance, we need [tex]\(10 \div 2 = 5\)[/tex] [tex]\(O_2\)[/tex] molecules.
[tex]\[ C_3H_8 + 5 O_2 \rightarrow 3 CO_2 + 4 H_2O \][/tex]
### Verification:
1. Count each type of atom on both sides of the equation:
- Reactants: [tex]\(C_3H_8 + 5 O_2\)[/tex]
- Carbon: 3
- Hydrogen: 8
- Oxygen: [tex]\(5 \times 2 = 10\)[/tex]
- Products: [tex]\(3 CO_2 + 4 H_2O\)[/tex]
- Carbon: 3
- Hydrogen: 8
- Oxygen: [tex]\(3 \times 2 + 4 \times 1 = 6 + 4 = 10\)[/tex]
All atoms balance correctly on both sides of the equation, verifying the equation is correct.
### Conclusion:
The balanced chemical equation for the burning of propane where all reactants and products are in the gas phase is:
[tex]\[ \boxed{C_3H_8(g) + 5 O_2(g) \rightarrow 3 CO_2(g) + 4 H_2O(g)} \][/tex]
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