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: An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at constant pressure of 30.0 atm and releases 67.9 kJ of heat. Before the r

Solution: An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at constant pressure of 30.0 atm and releases 67.9 kJ of heat. Before the r

Problem

An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at constant pressure of 30.0 atm and releases 67.9 kJ of heat. Before the reaction, the volume of the system was 8.00 L. After the reaction, the volume of the system was 2.80 L.

Calculate the total internal energy change, ΔE, in kilo joules.

Solution

We are being asked to calculate the internal energy in kilojoules (kJ) of the ideal gaseous reaction. 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:

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