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:
Hydrogen gas is produced when zinc reacts with sulfuric acid: Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)If 160 mL of wet H2 is collected over water at 24 oC and a barometric pressure of 738 torr, how many grams of Zn have been consumed? (The vapor pressure of water is 22.38 torr.)

Solution: Hydrogen gas is produced when zinc reacts with sulfuric acid:Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)If 160 mL of wet H2 is collected over water at 24 oC and a barometric pressure of 738 torr, how many g

Problem

Hydrogen gas is produced when zinc reacts with sulfuric acid:
Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)

If 160 mL of wet H2 is collected over water at 24 oC and a barometric pressure of 738 torr, how many grams of Zn have been consumed? (The vapor pressure of water is 22.38 torr.)