Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee all chapters
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 (C2H3OH) melts at-114°Cand boils at 78°C. The enthalpy of fusion of ethanol is 5.02 kJ/mol and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0 97 J/g • K are 2.3 J/g • K respectively.How much heat is required to convent 42.0 g of ethanol at -143 °C to the vapor phase at 78 °C? Express your answer using two significant figures.

Problem

Ethanol (C2H3OH) melts at-114°Cand boils at 78°C. The enthalpy of fusion of ethanol is 5.02 kJ/mol and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0 97 J/g • K are 2.3 J/g • K respectively.

How much heat is required to convent 42.0 g of ethanol at -143 °C to the vapor phase at 78 °C? Express your answer using two significant figures.

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