1.2 - Empirical and Molecular Formulas
Enroll to start learning
You’ve not yet enrolled in this course. Please enroll for free to listen to audio lessons, classroom podcasts and take practice test.
Practice Questions
Test your understanding with targeted questions
What is the empirical formula?
💡 Hint: Think of it as the reduced form of the chemical formula.
What does the molecular formula tell us?
💡 Hint: It's a complete version, unlike the empirical one.
4 more questions available
Interactive Quizzes
Quick quizzes to reinforce your learning
What is the ratio of elements in an empirical formula?
💡 Hint: Think of it as a simplified version of a chemical formula.
True or False: The molecular formula can be exactly the same as the empirical formula.
💡 Hint: Consider compounds where elements have the same ratios.
Get performance evaluation
Challenge Problems
Push your limits with advanced challenges
A compound is found to contain 35.0% Carbon, 7.0% Hydrogen, and 58.0% Oxygen by mass. Calculate both the empirical and molecular formulas given the molar mass is 180 g/mol.
💡 Hint: Convert mass percentages to moles, find ratios, then apply molar mass.
Given a compound composed of 10.0 g of Nitrogen and 30.0 g of Oxygen, find the empirical and molecular formulas given its molar mass of 90 g/mol.
💡 Hint: Use the masses to find moles, then ratios to find empirical, followed by molar mass for molecular.
Get performance evaluation
Reference links
Supplementary resources to enhance your learning experience.