Questions: After a reaction, a new compound contains 24.3 g Mg and 16.0 g O . What is the empirical formula of this compound? Use the equations interactive below to enter your answer.

After a reaction, a new compound contains 24.3 g Mg and 16.0 g O . What is the empirical formula of this compound? Use the equations interactive below to enter your answer.
Transcript text: After a reaction, a new compound contains 24.3 g Mg and 16.0 g O . What is the empirical formula of this compound? Use the equations interactive below to enter your answer.
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Solution

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Solution Steps

Step 1: Determine the Moles of Each Element
  • Given masses: 24.3 g of Mg and 16.0 g of O.
  • Molar mass of Mg = 24.305 g/mol.
  • Molar mass of O = 16.00 g/mol.

Calculate the moles of each element: \[ \text{Moles of Mg} = \frac{24.3 \text{ g}}{24.305 \text{ g/mol}} \approx 1.00 \text{ mol} \] \[ \text{Moles of O} = \frac{16.0 \text{ g}}{16.00 \text{ g/mol}} = 1.00 \text{ mol} \]

Step 2: Determine the Simplest Whole Number Ratio
  • The ratio of moles of Mg to moles of O is 1:1.
Step 3: Write the Empirical Formula
  • Since the ratio is 1:1, the empirical formula is MgO.

Final Answer

\[ \text{Empirical Formula} = \text{MgO} \]

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