Empirical and Molecular Formula Calculations
Chemistry ⇒ Stoichiometry and Chemical Calculations
Empirical and Molecular Formula Calculations starts at 10 and continues till grade 12.
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A compound contains 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. What is its empirical formula?
A compound contains 54.5% carbon, 9.1% hydrogen, and 36.4% oxygen. What is its empirical formula?
A compound contains 63.5% silver, 8.2% nitrogen, and 28.3% oxygen by mass. What is its empirical formula?
A compound contains 70% iron and 30% oxygen by mass. What is its empirical formula?
A compound has a molar mass of 58 g/mol and an empirical formula of C₂H₅. What is its molecular formula?
A compound has an empirical formula of CH₂ and a molar mass of 56 g/mol. What is its molecular formula?
A compound has the empirical formula C₂H₃O and a molar mass of 86 g/mol. What is its molecular formula?
A compound has the empirical formula NO₂ and a molar mass of 92 g/mol. What is its molecular formula?
A compound is found to contain 21.7% carbon, 9.6% hydrogen, and 68.7% oxygen by mass. If its molar mass is 90 g/mol, what is its molecular formula?
A compound is found to contain 36.5% sodium, 25.4% sulfur, and 38.1% oxygen by mass. What is its empirical formula?
A hydrocarbon has an empirical formula of CH and a molar mass of 78 g/mol. What is its molecular formula?
A sample of a compound contains 2.70 g of aluminum and 4.80 g of oxygen. What is the empirical formula of the compound?
Define empirical formula and explain how it differs from the molecular formula.
Describe the steps involved in determining the molecular formula of a compound from its empirical formula and molar mass.
Explain the significance of the empirical formula in chemical analysis.
Explain why ionic compounds are usually represented by their empirical formulas.
Explain why the empirical formula of a compound is not always the same as its molecular formula.
