Answer:
[tex]\large \boxed{1.615 \times 10^{25}\text{ molecules water}}[/tex]
Explanation:
You must calculate the mass of the water, convert it to moles, and then calculate the number of molecules.
1. Mass of water
[tex]\text{Mass } = \text{499.8 mL} \times \dfrac{\text{0.967 g}}{\text{1 mL}} = \text{483.3 g}[/tex]
2. Moles of water
[tex]\text{Moles of water} = \text{483.3 g water} \times \dfrac{\text{1 mol water}}{\text{18.02 g water}} = \text{26.82 mol water}[/tex]
3. Molecules of water
[tex]\text{No. of molecules} = \text{26.82 mol water} \times \dfrac{6.022 \times 10^{23}\text{ molecules water}}{\text{1 mol water}}\\\\= \mathbf{1.615 \times 10^{25}}\textbf{ molecules water}\\\text{The sample contains $\large \boxed{\mathbf{1.615 \times 10^{25}}\textbf{ molecules water}}$}[/tex]
The number of molecules of water present in the bottle is 1.62×10²⁵ molecules.
We'll begin by calculating the mass of the water in the bottle.
Mass = Density × Volume
Mass of water = 0.967 × 499.8
Mass of water = 483.3066 g
Finally, we shall determine number of molecules of water in the bottle.
From Avogadro's hypothesis,
1 mole of water = 6.02×10²³ molecules
But,
1 mole of water = 18 g
Thus, we can say that:
18 g of water = 6.02×10²³ molecules
Therefore,
483.3066 g of water = (483.3066 × 6.02×10²³) / 18
483.3066 g of water = 1.62×10²⁵ molecules
Thus, the number of molecules of water in the bottle is 1.62×10²⁵ molecules.
Learn more about Avogadro's number:
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