1 Multiple Choice 1 point A drop of water contains of molecules of $$ \mathrm{H}_{2} \mathrm{O} $$. millions trillions thousands billions

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To determine how many molecules of $$ \mathrm{H}_{2} \mathrm{O} $$ are in a drop of water, we can use the following information:

1. A typical drop of water has a volume of about $$ 0.05 $$ mL (milliliters).
2. The density of water is approximately $$ 1 \, \text{g/mL} $$, so $$ 0.05 \, \text{mL} $$ of water has a mass of about $$ 0.05 \, \text{g} $$.
3. The molar mass of water $$ \mathrm{H}_{2} \mathrm{O} $$ is approximately $$ 18 \, \text{g/mol} $$.
4. Using Avogadro's number, which is approximately $$ 6.022 \times 10^{23} $$ molecules/mol, we can calculate the number of molecules in the drop.

Now, let's calculate the number of molecules step by step:

1. Calculate the number of moles of water in the drop:
   $$
   \text{moles of } \mathrm{H}_{2} \mathrm{O} = \frac{\text{mass}}{\text{molar mass}} = \frac{0.05 \, \text{g}}{18 \, \text{g/mol}}
   $$

2. Calculate the number of molecules:
   $$
   \text{number of molecules} = \text{moles} \times \text{Avogadro's number}
   $$

Let's perform these calculations.

First, calculate the moles of water:
$$
\text{moles of } \mathrm{H}_{2} \mathrm{O} = \frac{0.05}{18} \approx 0.00278 \, \text{mol}
$$

Now, calculate the number of molecules:
$$
\text{number of molecules} = 0.00278 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol} \approx 1.67 \times 10^{21} \, \text{molecules}
$$

This value is in the range of billions (specifically, it is approximately 1.67 billion molecules).

Thus, the correct answer is:
**billions**.
A drop of water contains billions of $$ \mathrm{H}_{2} \mathrm{O} $$ molecules. **billions**

1 Multiple Choice 1 point A drop of water contains of molecules of \( \mathrm{H}_{2} \mathrm{O} \). millions trillions thousands billions

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