1st Law Of Thermodynamics - Chemistry LibreTexts

menu search Searchbuild_circle Toolbarfact_check Homeworkcancel Exit Reader Mode

• school Campus Bookshelves
• menu_book Bookshelves
• perm_media Learning Objects

• login Login
• how_to_reg Request Instructor Account
• hub Instructor Commons

Search

Search this book Submit Search

x

Text Color

Reset BrightBluesGrayInverted

Text Size

Reset +-

Margin Size

Reset +-

Font Type

Enable Dyslexic Font

• Downloads expand_more
  • Download Page (PDF)
  • Download Full Book (PDF)
• Resources expand_more
  • Periodic Table
  • Physics Constants
  • Scientific Calculator
• Reference expand_more
  • Reference & Cite
• Tools expand_more
• Help expand_more
  • Get Help
  • Feedback
  • Readability

x

selected template will load here

This action is not available.

chrome_reader_mode Enter Reader Mode The Four Laws of ThermodynamicsThermodynamics{ Conservation_of_Energy : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", First_Law_of_Thermodynamics : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()" }{ "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", "0th_Law_of_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", First_Law_of_Thermodynamics : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", Second_Law_of_Thermodynamics : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", Third_Law_of_Thermodynamics : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()" }{ Advanced_Thermodynamics : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", "Basics_Thermodynamics_(General_Chemistry)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", Calorimetry : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", Chemical_Energetics : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", Energies_and_Potentials : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", Fundamentals_of_Thermodynamics : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", Ideal_Systems : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", Path_Functions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", "Real_(Non-Ideal)_Systems" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", Thermochemistry : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", Thermodynamic_Cycles : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()", The_Four_Laws_of_Thermodynamics : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass234_0.<PageSubPageProperty>b__1]()" }Mon, 30 Jan 2023 07:57:29 GMT1st Law of Thermodynamics19201920admin{ }AnonymousAnonymous User2falsefalse[ "article:topic", "1st Law of Thermodynamics", "showtoc:no", "license:ccbyncsa", "licenseversion:40", "author@Lauren Boyle" ][ "article:topic", "1st Law of Thermodynamics", "showtoc:no", "license:ccbyncsa", "licenseversion:40", "author@Lauren Boyle" ]https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FPhysical_and_Theoretical_Chemistry_Textbook_Maps%2FSupplemental_Modules_(Physical_and_Theoretical_Chemistry)%2FThermodynamics%2FThe_Four_Laws_of_Thermodynamics%2FFirst_Law_of_Thermodynamics

• Sign in
• Forgot password

Search Search

• Home
• Bookshelves
• Physical & Theoretical Chemistry
• Supplemental Modules (Physical and Theoretical Chemistry)
• Thermodynamics
• The Four Laws of Thermodynamics

1st Law of Thermodynamics Last updated:

Page ID1920

\( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

\( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)

\( \newcommand{\dsum}{\displaystyle\sum\limits} \)

\( \newcommand{\dint}{\displaystyle\int\limits} \)

\( \newcommand{\dlim}{\displaystyle\lim\limits} \)

\( \newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\)

( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\)

\( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)

\( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\)

\( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)

\( \newcommand{\Span}{\mathrm{span}}\)

\( \newcommand{\id}{\mathrm{id}}\)

\( \newcommand{\Span}{\mathrm{span}}\)

\( \newcommand{\kernel}{\mathrm{null}\,}\)

\( \newcommand{\range}{\mathrm{range}\,}\)

\( \newcommand{\RealPart}{\mathrm{Re}}\)

\( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)

\( \newcommand{\Argument}{\mathrm{Arg}}\)

\( \newcommand{\norm}[1]{\| #1 \|}\)

\( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)

\( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\AA}{\unicode[.8,0]{x212B}}\)

\( \newcommand{\vectorA}[1]{\vec{#1}} % arrow\)

\( \newcommand{\vectorAt}[1]{\vec{\text{#1}}} % arrow\)

\( \newcommand{\vectorB}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

\( \newcommand{\vectorC}[1]{\textbf{#1}} \)

\( \newcommand{\vectorD}[1]{\overrightarrow{#1}} \)

\( \newcommand{\vectorDt}[1]{\overrightarrow{\text{#1}}} \)

\( \newcommand{\vectE}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{\mathbf {#1}}}} \)

\( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

\(\newcommand{\longvect}{\overrightarrow}\)

\( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)

\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\) Table of contents

1. Introduction
   1. Law of Thermodynamics
   2. Example \(\PageIndex{1}\)
   3. Example \(\PageIndex{2}\)
2. Outside Links
3. References
4. Contributors and Attributions

To understand and perform any sort of thermodynamic calculation, we must first understand the fundamental laws and concepts of thermodynamics. For example, work and heat are interrelated concepts. Heat is the transfer of thermal energy between two bodies that are at different temperatures and is not equal to thermal energy. Work is the force used to transfer energy between a system and its surroundings and is needed to create heat and the transfer of thermal energy. Both work and heat together allow systems to exchange energy. The relationship between the two concepts can be analyzed through the topic of Thermodynamics, which is the scientific study of the interaction of heat and other types of energy.

Introduction

To understand the relationship between work and heat, we need to understand a third, linking factor: the change in internal energy. Energy cannot be created nor destroyed, but it can be converted or transferred. Internal energy refers to all the energy within a given system, including the kinetic energy of molecules and the energy stored in all of the chemical bonds between molecules. With the interactions of heat, work and internal energy, there are energy transfers and conversions every time a change is made upon a system. However, no net energy is created or lost during these transfers.

Law of Thermodynamics

The First Law of Thermodynamics states that energy can be converted from one form to another with the interaction of heat, work and internal energy, but it cannot be created nor destroyed, under any circumstances. Mathematically, this is represented as

\[ \Delta U=q + w \label{1}\]

with

• \(ΔU\) is the total change in internal energy of a system,
• \(q\) is the heat exchanged between a system and its surroundings, and
• \(w\) is the work done by or on the system.

Work is also equal to the negative external pressure on the system multiplied by the change in volume:

\[ w=-p \Delta V \label{2}\]

where \(P\) is the external pressure on the system, and \(ΔV\) is the change in volume. This is specifically called "pressure-volume" work.

The internal energy of a system would decrease if the system gives off heat or does work. Therefore, internal energy of a system increases when the heat increases (this would be done by adding heat into a system). The internal energy would also increase if work were done onto a system. Any work or heat that goes into or out of a system changes the internal energy. However, since energy is never created nor destroyed (thus, the first law of thermodynamics), the change in internal energy always equals zero. If energy is lost by the system, then it is absorbed by the surroundings. If energy is absorbed into a system, then that energy was released by the surroundings:

\[\Delta U_{system} = -\Delta U_{surroundings} \]

where ΔUsystem is the total internal energy in a system, and ΔUsurroundingsis the total energy of the surroundings.

Table 1

Process	Sign of heat (q)	Sign of Work (w)
Work done by the system	N/A	-
Work done onto the system	N/A	+
Heat released from the system- exothermic (absorbed by surroundings)	-	N/A

The above figure is a visual example of the First Law of Thermodynamics. The blue cubes represent the system and the yellow circles represent the surroundings around the system. If energy is lost by the cube system then it is gained by the surroundings. Energy is never created nor destroyed. Since the area of the clue cube decreased the visual area of the yellow circle increased. This symbolizes how energy lost by a system is gained by the surroundings. The affects of different surroundings and changes on a system help determine the increase or decrease of internal energy, heat and work.

Table 2

The Process	Internal Energy Change	Heat Transfer of Thermal Energy (q)	Work (w=-PΔV)	Example
q=0 Adiabatic	+	0	+	Isolated system in which heat does not enter or leave similar to styrofoam
ΔV=0 Constant Volume	+	+	0	A hard, pressure isolated system like a bomb calorimeter
Constant Pressure	+ or -	enthalpy (ΔH)	-PΔV	Most processes occur are constant external pressure
ΔT=0 Isothermal	0	+	-	There is no change in temperature like in a temperature bath

Example \(\PageIndex{1}\)

A gas in a system has constant pressure. The surroundings around the system lose 62 J of heat and does 474 J of work onto the system. What is the internal energy of the system?

Solution

To find internal energy, ΔU, we must consider the relationship between the system and the surroundings. Since the First Law of Thermodynamics states that energy is not created nor destroyed we know that anything lost by the surroundings is gained by the system. The surrounding area loses heat and does work onto the system. Therefore, q and w are positive in the equation ΔU=q+w because the system gains heat and gets work done on itself.

\[\begin{align} ΔU &= (62\,J) + (474\,J) \\[4pt] &= 536\,J \end{align}\]

Example \(\PageIndex{2}\)

A system has constant volume (ΔV=0) and the heat around the system increases by 45 J.

1. What is the sign for heat (q) for the system?
2. What is ΔU equal to?
3. What is the value of internal energy of the system in Joules?

Solution

Since the system has constant volume (ΔV=0) the term -PΔV=0 and work is equal to zero. Thus, in the equation ΔU=q+w w=0 and ΔU=q. The internal energy is equal to the heat of the system. The surrounding heat increases, so the heat of the system decreases because heat is not created nor destroyed. Therefore, heat is taken away from the system making it exothermic and negative. The value of Internal Energy will be the negative value of the heat absorbed by the surroundings.

1. negative (q<0)
2. ΔU=q + (-PΔV) = q+ 0 = q
3. ΔU = -45J

Outside Links

• Hamby, Marcy. "Understanding the language: Problem solving and the first law of thermodynamics." J. Chem. Educ. 1990: 67, 923.

References

1. Chang, Raymond. Chemistry: Ninth Edition
2. Petrucci, Harwood, Herring, Madura.General Chemistry: Ninth Edition

Contributors and Attributions

• Lauren Boyle (UCD)

1st Law of Thermodynamics is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Lauren Boyle.

1. Back to top
2. • 0th Law of Thermodynamics
   • Conservation of Energy

1. © Copyright 2026 Chemistry LibreTexts
2. Powered by CXone Expert ®

The LibreTexts libraries are Powered by NICE CXone Expert and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Privacy Policy. Terms & Conditions. Accessibility Statement. For more information contact us at [email protected].