Questions: A compound with the empirical formula of CH4O and a molar mass of 32 g/mol has a molecular formula of: Select the correct answer below: CH4O C2H8O2 C2H4O2 C3H8O3

A compound with the empirical formula of CH4O and a molar mass of 32 g/mol has a molecular formula of: Select the correct answer below: CH4O C2H8O2 C2H4O2 C3H8O3
Transcript text: A compound with the empirical formula of $\mathrm{CH}_{4} \mathrm{O}$ and a molar mass of $32 \mathrm{~g} / \mathrm{mol}$ has a molecular formula of: Select the correct answer below: $\mathrm{CH}_{4} \mathrm{O}$ $\mathrm{C}_{2} \mathrm{H}_{8} \mathrm{O}_{2}$ $\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}$ $\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}_{3}$
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Solution

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Solution Steps

Step 1: Determine the Molar Mass of the Empirical Formula

The empirical formula given is \(\mathrm{CH}_4\mathrm{O}\). To find its molar mass, we calculate the sum of the atomic masses of each element in the formula:

  • Carbon (C): \(12.01 \, \text{g/mol}\)
  • Hydrogen (H): \(1.008 \, \text{g/mol} \times 4 = 4.032 \, \text{g/mol}\)
  • Oxygen (O): \(16.00 \, \text{g/mol}\)

Adding these together gives: \[ 12.01 + 4.032 + 16.00 = 32.042 \, \text{g/mol} \]

Step 2: Compare Empirical Formula Molar Mass with Given Molar Mass

The molar mass of the empirical formula \(\mathrm{CH}_4\mathrm{O}\) is \(32.042 \, \text{g/mol}\), which is approximately equal to the given molar mass of the compound, \(32 \, \text{g/mol}\).

Step 3: Determine the Molecular Formula

Since the molar mass of the empirical formula matches the given molar mass of the compound, the empirical formula is also the molecular formula.

Final Answer

\[ \boxed{\mathrm{CH}_4\mathrm{O}} \]

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