To determine the product of the given chemical equation, we first write the balanced chemical equation for the combustion of propane (\( C_3H_8 \)):
[tex]\[ C_3H_8(g) + 5 O_2(g) \rightarrow 3 CO_2(g) + 4 H_2O(g) \][/tex]
Now let's break this down step-by-step:
1. Identification of reactants: The reactants in the equation are propane (\( C_3H_8 \)) and oxygen (\( O_2 \)).
2. Combustion reaction overview: Combustion reactions involving hydrocarbons (compounds composed of carbon and hydrogen) in the presence of sufficient oxygen typically produce carbon dioxide (\( CO_2 \)) and water (\( H_2O \)).
3. Balancing the equation: To verify that the equation is balanced:
- Count the number of atoms of each element on both sides of the equation.
- On the reactant side:
- Carbon (\( C \)): 3 atoms (from \( C_3H_8 \))
- Hydrogen (\( H \)): 8 atoms (from \( C_3H_8 \))
- Oxygen (\( O \)): 10 atoms (from 5 \( O_2 \))
- On the product side:
- Carbon (\( C \)): 3 atoms (from 3 \( CO_2 \))
- Hydrogen (\( H \)): 8 atoms (from 4 \( H_2O \))
- Oxygen (\( O \)): 10 atoms (6 from 3 \( CO_2 \) and 4 from 4 \( H_2O \))
Since the number of each type of atom is equal on both sides of the chemical equation, the equation is balanced.
4. Final products: The balanced chemical equation tells us that the products are carbon dioxide (\( CO_2 \)) and water (\( H_2O \)).
Given this analysis, the correct answer is:
B. carbon dioxide and water
