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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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.
Which of the following best describes the process to determine an empirical formula from percent composition? (1) Convert percentages to grams, then to moles, divide by the smallest number of moles, and round to the nearest whole number. (2) Add the percentages and divide by the molar mass. (3) Multiply the percentages by the atomic number.
Which of the following is NOT an empirical formula? (1) C₂H₄ (2) CH₂ (3) NO₂ (4) H₂O
Which of the following is the correct empirical formula for a compound with 80% carbon and 20% hydrogen by mass? (1) CH (2) C₂H₅ (3) CH₃ (4) C₄H₁₀
Which of the following is the correct empirical formula for a compound with the molecular formula C₈H₁₈? (1) C₄H₉ (2) C₂H₅ (3) C₈H₁₈ (4) CH₂.₂₅
Fill in the blank: The empirical formula of C₄H₁₀ is __________.
Fill in the blank: The empirical formula of C₆H₁₄ is __________.
Fill in the blank: The empirical formula of C₉H₁₈O₃ is __________.
Fill in the blank: The empirical formula of hydrogen peroxide (H₂O₂) is __________.
True or False: The empirical formula of a compound can be determined from its molecular formula.
True or False: The empirical formula of a compound can be determined from its percent composition by mass.
True or False: The empirical formula of a compound is always unique for that compound.
True or False: The empirical formula of glucose (C₆H₁₂O₆) is CH₂O.
