How many molecules of water are produced by the complete combustion of 3.00 g of methane (CH_4)?

• A. 6.02 × 10^{22} molecules
• B. 1.13 × 10^{23} molecules
• C. 4.52 × 10^{23} molecules
• D. 2.26 × 10^{23} molecules

Answer: (D)

Verified step by step guidance

1. Write the balanced chemical equation for the complete combustion of methane (CH_4): \(\mathrm{CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O}\).
2. Calculate the number of moles of methane in 3.00 g using its molar mass. The molar mass of methane (CH_4) is calculated as \$12.01 + 4 \times 1.008\( g/mol. Use the formula: \)\text{moles of CH}_4 = \frac{\text{mass of CH}_4}{\text{molar mass of CH}_4}$.
3. Use the mole ratio from the balanced equation to find the moles of water produced. According to the equation, 1 mole of CH_4 produces 2 moles of H_2O, so multiply the moles of CH_4 by 2.
4. Convert the moles of water to molecules using Avogadro's number, \$6.022 \times 10^{23}\( molecules/mol. Use the formula: \)\text{molecules of H}_2\text{O} = \text{moles of H}_2\text{O} \times 6.022 \times 10^{23}$.
5. Compare your calculated number of water molecules to the given options to identify the correct answer.