Identify each energy exchange as primarily heat or work and determine whether the sign of ΔE is positive or negative for the system. Identify each energy exchange as primarily heat or work. a. A rolling billiard ball collides with another billiard ball. The first billiard ball (defined as the system) stops rolling after the collision. b. A book falls to the floor. (The book is the system). c. A father pushes his daughter on a swing. (The daughter and the swing are the system). Identify each energy exchange as primarily heat or work.

Key Concepts

First Law of Thermodynamics

The First Law of Thermodynamics states that energy cannot be created or destroyed, only transformed from one form to another. This principle is crucial for analyzing energy exchanges in systems, as it helps determine how energy is conserved during processes like collisions or movements. Understanding this law allows us to assess whether energy is being added to or removed from a system, which is essential for evaluating the sign of ΔE.

Heat vs. Work

In thermodynamics, heat and work are two distinct forms of energy transfer. Heat refers to energy transferred due to a temperature difference, while work is energy transferred when a force is applied over a distance. Identifying whether an energy exchange is primarily heat or work is vital for understanding how energy flows in a system and affects its internal energy, ΔE.

Sign Convention for ΔE

The sign of ΔE, or the change in internal energy of a system, indicates whether the system has gained or lost energy. A positive ΔE means the system has gained energy (e.g., through heat absorption or work done on it), while a negative ΔE indicates energy loss. This convention is essential for interpreting the outcomes of energy exchanges in various scenarios, such as collisions or mechanical work.