Ch.3 - Chemical ReactionsSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Combustion analysis of a 12.01 g sample of tartaric acid, which contains only  carbon, hydrogen, and oxygen, produced 14.08 g CO2 and 4.32 g H2O. a) What is the empirical formula of tartaric acid?             b) If 0.250 moles of the compound weighs 37.52 g, what is the molecular formula of the compound?  

Problem

Combustion analysis of a 12.01 g sample of tartaric acid, which contains only  carbon, hydrogen, and oxygen, produced 14.08 g CO2 and 4.32 g H2O.

a) What is the empirical formula of tartaric acid?

 

 



 

 

 

 

b) If 0.250 moles of the compound weighs 37.52 g, what is the molecular formula of the compound?