Ch.6 - Thermochemistry WorksheetSee 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: Calculate the enthalpy of methanol (CH3OH(l) (MW = 32.0 g/mol), if a 2.885 g sample of methanol is burned in a bomb calorimeter (Kc = 727.1 J/°C) containing 1.200 kg of water (Cp = 4.184 J/°C). The te

Problem

Calculate the enthalpy of methanol (CH3OH(l) (MW = 32.0 g/mol), if a 2.885 g sample of methanol is burned in a bomb calorimeter (Kc = 727.1 J/°C) containing 1.200 kg of water (Cp = 4.184 J/°C). The temperature of the calorimeter increases by 11.38°C. 

a. 635 kJ/mol

b. -1.02 x 106 kJ/mol 

c. -726 kJ/mol  

d. -91.9 kJ/mol  

e. -65.4 kJ/mol