To find the number of moles of [tex]\( H_2O \)[/tex] that contain 16 grams of oxygen, we need to consider the molar masses of the elements involved and the composition of water.
1. Determine the molar mass of [tex]\( H_2O \)[/tex]:
- The molar mass of hydrogen (H) is 1 g/mol.
- Each water molecule ([tex]\( H_2O \)[/tex]) consists of two hydrogen atoms.
- Therefore, the total mass of hydrogen in one mole of water is [tex]\( 2 \times 1 \text{ g/mol} = 2 \text{ g/mol} \)[/tex].
- The molar mass of oxygen (O) is 16 g/mol.
- Adding these together, the molar mass of [tex]\( H_2O \)[/tex] is [tex]\( 2 \text{ g/mol (H)} + 16 \text{ g/mol (O)} = 18 \text{ g/mol} \)[/tex].
2. Given mass of oxygen:
- We have 16 grams of oxygen.
3. Calculate the moles of [tex]\( H_2O \)[/tex] equivalent to the given mass of oxygen:
- From the stoichiometry of water, 1 mole of [tex]\( H_2O \)[/tex] contains 1 mole of oxygen.
- Hence, the molar mass ratio will allow us to determine the total moles of water.
4. Calculation:
[tex]\[
\text{Moles of } H_2O = \frac{\text{Mass of O}}{\text{Molar mass of } H_2O} = \frac{16 \text{ g}}{18 \text{ g/mol}} = 0.8888888... \approx 0.89 \text{ moles}
\][/tex]
Given the context of the problem and the available options,
- X. 1.0
- C. 0.25
- B. 0.5
- D. 0.1
The closest and most appropriate choice is approximately 0.89.
Therefore, the number of moles of [tex]\( H_2O \)[/tex] that contains 16 g of oxygen is approximately [tex]\( 0.89 \)[/tex], which is given by:
[tex]\[
\boxed{0.88}
\][/tex]
Among the options provided, there seems to be no exact match for 0.88. However, Option X (1.0) being the closest indicates that an approximation or context consideration is likely proper in context. To be consistent with the problem format above, assume approximations meant closest value match.
So the final choice is option [tex]\( X: 1.0 \)[/tex] (or something like being prompted as closest if instruction adaptation applied).
