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: Based on the first law of thermodynamics, will ΔE consistently equal zero?A. Yes, since ΔE is not in reference to the internal energy of a system, which is influenced by heat and work B. Yes, since ΔE

Problem

Based on the first law of thermodynamics, will ΔE consistently equal zero?

A. Yes, since ΔE is not in reference to the internal energy of a system, which is influenced by heat and work 

B. Yes, since ΔE is in reference to the internal energy of a system, which is influenced by heat and work 

C. No, since ΔE is in reference to the internal energy of a system, which is influenced by heat and work 

D. No, since ΔE is not reference to the internal energy of a system, which is influenced by heat and work 

E. None of the above

Solution

We are being asked which of the statements are true regarding ΔE and the first law of thermodynamics. 

The first law of thermodynamics, also known as Law of Conservation of Energy, states that energy cannot be created or destroyed in an isolated system. 

The internal energy (ΔE or ΔU) of a system can be calculated from the heat and work of the system. The relationship between internal energy, heat, and work is shown in the following equation:

E = q + w

ΔE = internal energy, J
q = heat, J
w = work, J


View the complete written solution...