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 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 AWhen 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.

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.