General Chemistry 2 Thermodynamics Quiz and Flashcards

Study Notes

Thermodynamics and Energy Transfer

Thermodynamics is the scientific study of the interaction of heat and other types of energy.
Heat energy flows from higher temperature to lower temperature.
Work done by a system is defined as the quantity of energy exchanged between a system and its surroundings.

Internal Energy

Internal energy refers to all the energy within a given system, including kinetic energy of molecules and energy stored in chemical bonds.
The internal energy of a system may change when:
- Heat passes into or out of the system.
- Work is done on or by the system.
- Matter enters or leaves the system.
Work done BY System is negative, while work done ON System is positive.

Thermodynamic System and Surrounding

A system is the part of the universe under study where observations are made.
The surrounding and universe interact with each other, exchanging energy and matter.
There are three types of systems:
- Open System: allows exchange of energy and matter.
- Closed System: allows only energy exchange, but not matter.
- Isolated System: neither energy nor matter can be exchanged.

Energy Transfer

Energy transfer occurs in chemical reactions due to absorption or release of energy when chemical bonds are broken or formed.
The Law of Conservation of Energy states that the total energy of a system must remain unchanged.
Energy transfer can be classified as:
- Exothermic Reaction: releases heat and light into surroundings (e.g., combustion reactions).
- Endothermic Reaction: absorbs heat and/or light from surroundings (e.g., decomposition reactions).

Enthalpy

Enthalpy is the measurement of energy in a thermodynamic system.
Enthalpy is the total content of heat of a system, equivalent to the system's internal energy plus the product of volume and pressure.
The flow of heat (q) at constant pressure in a process equals the change in enthalpy.

Laws of Thermodynamics

1st Law of Thermodynamics (Law of Conservation of Energy): energy can neither be created nor destroyed, but it can be changed from one form to another.
The law can be represented mathematically as: ΔU = ΔQ + W
Where ΔQ is the heat given or lost, ΔU is the change in internal energy, and W is the work done.

Description

Test your understanding of thermodynamics and chemical thermodynamics concepts, including energy transfer, the laws of thermodynamics, enthalpy, entropy, and Gibbs free energy. This quiz covers topics from Module 5 and 6 of General Chemistry 2.