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: Ethanol, C2H5OH, is produced industrially from ethylene, C2H4, by the following sequence of reactions:3C2H4 + 2 H2SO4 ⟶ C2H5HSO4 + (C2H5)2SO4 C2H5HSO4 + (C2H5)2SO4 + 3 H2O ⟶ 3 C2H5OH + 2 H2SO4What vol

Problem

Ethanol, C2H5OH, is produced industrially from ethylene, C2H4, by the following sequence of reactions:

3C2H4 + 2 H2SO4 ⟶ C2H5HSO4 + (C2H5)2SO4 

C2H5HSO4 + (C2H5)2SO4 + 3 H2O ⟶ 3 C2H5OH + 2 H2SO4

What volume of ethylene at STP is required to produce 1.000 metric ton (1000 kg) of ethanol if the overall yield of ethanol is 90.1%?