A sample of water has a volume of 10.0 cm^3. Given that the density of water is 1.0 g/cm^3, how many water molecules are present in the sample? (Molar mass of H_2O = 18.0 g/mol; Avogadro's number = 6.02 × 10^{23} molecules/mol)

• A. 3.34 × 10^{23} molecules
• B. 5.56 × 10^{22} molecules
• C. 6.02 × 10^{22} molecules
• D. 1.80 × 10^{24} molecules

Answer: (A)

Verified step by step guidance

1. Calculate the mass of the water sample using the formula for density: \(\text{mass} = \text{density} \times \text{volume}\). Given density is 1.0 g/cm\(^{3}\) and volume is 10.0 cm\(^{3}\), find the mass in grams.
2. Convert the mass of water to moles using the molar mass of water. Use the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\), where the molar mass of H\(_2\)O is 18.0 g/mol.
3. Calculate the number of water molecules by multiplying the number of moles by Avogadro's number. Use the formula: \(\text{number of molecules} = \text{moles} \times \text{Avogadro's number}\), where Avogadro's number is \$6.02 \times 10^{23}$ molecules/mol.
4. Make sure to keep track of units throughout the calculations to ensure consistency and correctness.
5. Express the final answer in scientific notation to match the format of the given options.