Given the reaction 2H2O + 2F2 → 4HF + O2, what mass of fluorine (F2) is needed to completely react with 3.6 grams of water (H2O)?

• A. 6.0 grams
• B. 3.2 grams
• C. 4.0 grams
• D. 8.0 grams

Answer: (A)

Verified step by step guidance

1. Write down the balanced chemical equation: \$2H_2O + 2F_2 \rightarrow 4HF + O_2$.
2. Calculate the number of moles of water (H\(_2\)O) given its mass. Use the molar mass of water, which is approximately 18.0 g/mol, and apply the formula: \(\text{moles of } H_2O = \frac{\text{mass of } H_2O}{\text{molar mass of } H_2O}\).
3. Use the stoichiometric coefficients from the balanced equation to find the moles of fluorine (F\(_2\)) needed. According to the equation, 2 moles of H\(_2\)O react with 2 moles of F\(_2\), so the mole ratio is 1:1.
4. Calculate the mass of fluorine required by multiplying the moles of F\(_2\) by its molar mass (approximately 38.0 g/mol): \(\text{mass of } F_2 = \text{moles of } F_2 \times \text{molar mass of } F_2\).
5. Summarize the process: convert grams of water to moles, use mole ratio to find moles of fluorine, then convert moles of fluorine to grams to find the required mass.