This is “Energy”, section 7.1 from the book Beginning Chemistry (v. 1.0).
This book is licensed under a Creative Commons by-nc-sa 3.0 license. See the license for more details, but that basically means you can share this book as long as you credit the author (but see below), don't make money from it, and do make it available to everyone else under the same terms.
This content was accessible as of December 29, 2012, and it was downloaded then by Andy Schmitz in an effort to preserve the availability of this book.
Normally, the author and publisher would be credited here. However, the publisher has asked for the customary Creative Commons attribution to the original publisher, authors, title, and book URI to be removed. Additionally, per the publisher's request, their name has been removed in some passages. More information is available on this project's attribution page.
For more information on the source of this book, or why it is available for free, please see the project's home page. You can browse or download additional books there. You may also download a PDF copy of this book (40 MB) or just this chapter (1 MB), suitable for printing or most e-readers, or a .zip file containing this book's HTML files (for use in a web browser offline).
EnergyThe ability to do work. is the ability to do work. Think about it: when you have a lot of energy, you can do a lot of work; but if you’re low on energy, you don’t want to do much work. Work (w) itself is defined as a force (F) operating over a distance (Δx):w = F × Δx
In SI, force has units of newtons (N), while distance has units of meters. Therefore, work has units of N·m. This compound unit is redefined as a jouleThe SI unit of energy. (J):1 joule = 1 newton·meter 1 J = 1 N·m
Because energy is the ability to do work, energy is also measured in joules. This is the primary unit of energy we will use here.
How much is 1 J? It is enough to warm up about one-fourth of a gram of water by 1°C. It takes about 12,000 J to warm a cup of coffee from room temperature to 50°C. So a joule is not a lot of energy. It will not be uncommon to measure energies in thousands of joules, so the kilojoule (kJ) is a common unit of energy, with 1 kJ equal to 1,000 J.
An older—but still common—unit of energy is the calorie. The calorie (cal) was originally defined in terms of warming up a given quantity of water. The modern definition of calorie equates it to joules:1 cal = 4.184 J
One area where the calorie is used is in nutrition. Energy contents of foods are often expressed in calories. However, the calorie unit used for foods is actually the kilocalorie (kcal). Most foods indicate this by spelling the word with a capital C—Calorie. Figure 7.1 "Calories on Food Labels" shows one example. So be careful counting calories when you eat!
Figure 7.1 Calories on Food Labels
This label expresses the energy content of the food, but in Calories (which are actually kilocalories).
The label in Figure 7.1 "Calories on Food Labels" states that the serving has 38 Cal. How many joules is this?
We recognize that with a capital C, the Calories unit is actually kilocalories. To determine the number of joules, we convert first from kilocalories to calories (using the definition of the kilo- prefix) and then from calories to joules (using the relationship between calories and joules). So
A serving of breakfast cereal usually has 110 Cal. How many joules of energy is this?
In the study of energy, we use the term systemThe part of the universe under study. to describe the part of the universe under study: a beaker, a flask, or a container whose contents are being observed and measured. An isolated systemA system that does not allow a transfer of energy or matter into or out of the system. is a system that does not allow a transfer of energy or matter into or out of the system. A good approximation of an isolated system is a closed, insulated thermos-type bottle. The fact that the thermos-type bottle is closed keeps matter from moving in or out, and the fact that it is insulated keeps energy from moving in or out.
One of the fundamental ideas about the total energy of an isolated system is that is does not increase or decrease. When this happens to a quantity, we say that the quantity is conserved. The statement that the total energy of an isolated system does not change is called the law of conservation of energyThe total energy of an isolated system does not increase or decrease.. As a scientific law, this concept occupies the highest level of understanding we have about the natural universe.
Define energy. How is work related to energy?
Give two units of energy and indicate which one is preferred.
Express the quantity of 422 J in calories.
Express the quantity of 3.225 kJ in calories.
Express the quantity 55.69 cal in joules.
Express the quantity 965.33 kcal in joules.
How does a Calorie differ from a calorie?
Express the quantity 965.33 Cal in joules.
What is the law of conservation of energy?
What does the word conserved mean as applied to the law of conservation of energy?
Energy is the ability to do work. Work is a form of energy.
A Calorie is actually a kilocalorie, or 1,000 calories.
The total energy of an isolated system does not increase or decrease.