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: A chemist measures the energy change ΔH during the following reaction: CH4 (g)+2O2 (g) → CO2 (g) + 2H2O (l)     ΔH = -882. kJUse the information to answer the following questions. The reaction is:   


A chemist measures the energy change ΔH during the following reaction: 

CH4 (g)+2O2 (g) → CO2 (g) + 2H2O (l)     ΔH = -882. kJ

Use the information to answer the following questions. 

The reaction is:

                   (i) endothermic. 

                   (ii) exothermic. 

Suppose 84.2 g of CH4 react. Will any heat be released or absorbed?

                   (i) Yes, absorbed. 

                   (ii) Yes, released. 

                   (iii) No. 

If you said heat will be released or absorbed in the second part of this question, calculate how much heat in kJ will be released or absorbed. Round your answer to 3 significant digits.

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