Multiple Choice
Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.
3. Chemical Reactions
Empirical Formula
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In an experiment, 10.0 g of sulfur and 10.0 g of oxygen react completely to form an oxide of sulfur. What is its empirical formula?
A
S2O3
B
S2O
C
SO2
D
SO
Verified step by step guidance1
Determine the number of moles of sulfur (S) by using its molar mass. The molar mass of sulfur is approximately 32.07 g/mol. Use the formula: \( \text{moles of S} = \frac{\text{mass of S}}{\text{molar mass of S}} \).
Determine the number of moles of oxygen (O) by using its molar mass. The molar mass of oxygen is approximately 16.00 g/mol. Use the formula: \( \text{moles of O} = \frac{\text{mass of O}}{\text{molar mass of O}} \).
Calculate the mole ratio of sulfur to oxygen by dividing the number of moles of each element by the smallest number of moles calculated in the previous steps.
Simplify the mole ratio to the smallest whole numbers to determine the empirical formula. This involves dividing each mole value by the smallest mole value obtained.
Write the empirical formula using the simplified whole number ratio of sulfur to oxygen. This will give you the simplest whole number ratio of atoms in the compound.
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