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: Cavendish prepared hydrogen in 1766 by the novel method of passing steam through a red-hot gun barrel:4 H2O (g) + 3 Fe(s) ⟶ Fe3O4 (s) + 4 H2 (g) (a) Outline the steps necessary to answer the following

Solution: Cavendish prepared hydrogen in 1766 by the novel method of passing steam through a red-hot gun barrel:4 H2O (g) + 3 Fe(s) ⟶ Fe3O4 (s) + 4 H2 (g) (a) Outline the steps necessary to answer the following

Problem

Cavendish prepared hydrogen in 1766 by the novel method of passing steam through a red-hot gun barrel:

4 H2O (g) + 3 Fe(s) ⟶ Fe3O4 (s) + 4 H2 (g) 

(a) Outline the steps necessary to answer the following question: What volume of H2 at a pressure of 745 torr and a temperature of 20 °C can be prepared from the reaction of 15.0 g of H2O?

Solution

We can use the ideal gas law to determine the volume of H2 produced by the reaction.

We first need to determine the moles of H2 produced from 15.0 g H2O. The molar mass of H2O is 2(1.01 g/mol H) + 16.00 g/mol O = 18.02 g/mol. From the given chemical equation, 4 moles of H2O form 4 moles of H2.

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