To determine the mass of [tex]\(H_2O\)[/tex] formed during the reaction using the Law of Conservation of Mass, we will follow these steps:
1. Understand the given data:
- Mass of [tex]\(CH_4\)[/tex] (Methane) is 16 grams.
- Mass of [tex]\(O_2\)[/tex] (Oxygen) is 64 grams.
- Mass of [tex]\(CO_2\)[/tex] (Carbon Dioxide) is 44 grams.
- We need to find the mass of [tex]\(H_2O\)[/tex] (Water).
2. Apply the Law of Conservation of Mass:
The Law of Conservation of Mass states that the total mass of reactants must equal the total mass of products.
3. Calculate the total mass of reactants:
[tex]\[
\text{Total mass of reactants} = \text{Mass of } CH_4 + \text{Mass of } O_2
\][/tex]
Substituting the given values:
[tex]\[
\text{Total mass of reactants} = 16 \, \text{g} + 64 \, \text{g} = 80 \, \text{g}
\][/tex]
4. Set up the equation for mass conservation:
[tex]\[
\text{Total mass of reactants} = \text{Total mass of products}
\][/tex]
Let [tex]\(X\)[/tex] be the mass of [tex]\(H_2O\)[/tex]:
[tex]\[
80 \, \text{g} = 44 \, \text{g} + X
\][/tex]
5. Solve for the mass of [tex]\(H_2O\)[/tex]:
[tex]\[
X = 80 \, \text{g} - 44 \, \text{g}
\][/tex]
[tex]\[
X = 36 \, \text{g}
\][/tex]
Therefore, the mass of [tex]\(H_2O\)[/tex] produced during the reaction is 36 grams.
