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: The ideal gas law PV = nRT relates pressure P, volume V, temperature T, and number of moles of a gas, n. The gas constant R equals 0.08208 L middot atm/(K • mol) or 8.3145 J/(K • mol). The equation ca

Problem

The ideal gas law 

PV = nRT 

relates pressure P, volume V, temperature T, and number of moles of a gas, n. The gas constant R equals 0.08208 L middot atm/(K • mol) or 8.3145 J/(K • mol). The equation can be rearranged as follows to for n: 

n = PV/RT 

This equation is useful when dealing with gaseous because calculations involve mole ratios. 

Part A

When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction 

CaCO3  → CaO + CO2  

What is the mass of calcium carbonate needed to produce 63.0 L of carbon dioxide at STP? 

Express your answer with the appropriate units.