Asked by lo
A sample of a compound contains 60.0 g C and 5.05 g H. Its molar mass is 78.12 g/mol. What is the compound’s molecular formula?
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1) Find moles of each element (using atomic masses C = 12.01, H = 1.008):
- moles C = 60.0 g / 12.01 g·mol⁻¹ = 4.996 mol
- moles H = 5.05 g / 1.008 g·mol⁻¹ = 5.010 mol
2) Ratio C : H ≈ 4.996 : 5.010 ≈ 1.00 : 1.00 → empirical formula = CH.
3) Empirical formula mass = 12.01 + 1.008 = 13.018 g·mol⁻¹.
n = molar mass / empirical mass = 78.12 / 13.018 ≈ 6.00
4) Molecular formula = (CH)6 = C6H6.
Answer: C6H6 (benzene).
- moles C = 60.0 g / 12.01 g·mol⁻¹ = 4.996 mol
- moles H = 5.05 g / 1.008 g·mol⁻¹ = 5.010 mol
2) Ratio C : H ≈ 4.996 : 5.010 ≈ 1.00 : 1.00 → empirical formula = CH.
3) Empirical formula mass = 12.01 + 1.008 = 13.018 g·mol⁻¹.
n = molar mass / empirical mass = 78.12 / 13.018 ≈ 6.00
4) Molecular formula = (CH)6 = C6H6.
Answer: C6H6 (benzene).
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