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: What volume of CO2 gas (MM = 44.01 g/mol) can be produced from the reaction of 2.00 L of 1.00 M HCl reacting with excess CaCO3 at standard temperature and pressure?  2 HCl (aq) + CaCO3 (s) → CO2 (g) + H2O(l) + CaCl2 (aq)A.  0.509 L        B.  2.00 L        C.  4.00 L        D.  22.4 L        E.  44.8 L

Problem

What volume of CO2 gas (MM = 44.01 g/mol) can be produced from the reaction of 2.00 L of 1.00 M HCl reacting with excess CaCO3 at standard temperature and pressure?  

2 HCl (aq) + CaCO3 (s) → CO2 (g) + H2O(l) + CaCl2 (aq)

A.  0.509 L        

B.  2.00 L        

C.  4.00 L        

D.  22.4 L        

E.  44.8 L