Multiple Choice
Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.
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3. Chemical Reactions
Empirical Formula
Multiple Choice
If 0.500 mol of copper combines with 0.250 mol of sulfur, what is the empirical formula of the copper sulfide product?
A
Cu5S5
B
CuS
C
CuS2
D
Cu2S
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Verified step by step guidance1
Determine the mole ratio of copper to sulfur by dividing the number of moles of each element by the smallest number of moles present. In this case, divide both 0.500 mol of copper and 0.250 mol of sulfur by 0.250 mol.
Calculate the ratio for copper: \( \frac{0.500 \text{ mol Cu}}{0.250 \text{ mol}} = 2 \).
Calculate the ratio for sulfur: \( \frac{0.250 \text{ mol S}}{0.250 \text{ mol}} = 1 \).
Use the mole ratios to write the empirical formula. The ratio of copper to sulfur is 2:1, which means there are 2 copper atoms for every sulfur atom.
Write the empirical formula based on the ratio: \( \text{Cu}_2\text{S} \).
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