To determine the number of moles of hydrogen atoms in a sample containing 4,786.4 mg of C₆H₉O, follow these steps:

1. Convert mass from mg to grams:

$4,786.4 \, \text{mg} = 4.7864 \, \text{g}$

2. Find the molar mass of C₆H₉O:

• Carbon (C): $6 \times 12.01 \, \text{g/mol} = 72.06 \, \text{g/mol}$
• Hydrogen (H): $9 \times 1.008 \, \text{g/mol} = 9.072 \, \text{g/mol}$
• Oxygen (O): $1 \times 16.00 \, \text{g/mol} = 16.00 \, \text{g/mol}$

Thus, the molar mass of C₆H₉O is: $72.06 + 9.072 + 16.00 = 97.132 \, \text{g/mol}$

3. Calculate the number of moles of C₆H₉O:

$\text{Moles of C₆H₉O} = \frac{4.7864 \, \text{g}}{97.132 \, \text{g/mol}} = 0.04928 \, \text{mol}$

4. Determine the number of moles of hydrogen atoms:

Each molecule of C₆H₉O contains 9 hydrogen atoms. Therefore, the number of moles of hydrogen atoms is: $\text{Moles of H atoms} = 0.04928 \, \text{mol C₆H₉O} \times 9 = 0.4435 \, \text{mol}$

Thus, the sample contains 0.4435 moles of hydrogen atoms.

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Related Questions:

1. How do you calculate the molar mass of a compound with multiple elements?
2. What are moles, and why are they important in chemistry?
3. How do you convert between mass and moles?
4. What is Avogadro's number, and how is it related to moles?
5. How would the calculation change if the compound contained isotopes of hydrogen?

Tip:

Always double-check your units when converting between mass and moles to avoid errors in the calculation!