Name: enthalpy and heat at constant pressure
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 59 s
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PS.Chm.7.2

Enthalpy

תגובות כימיות מסוימות משחררות חום אדיר ומבצעות עבודה על הסביבה. לדוגמה, הבערה של דלק טילים, הגורמת לחללית להמריא מעל פני האדמה. סכום החום, Q, והעבודה, W, הוא השינוי באנרגיה הפנימית, ΔE(דלתא E)כפי שמוצג בחוק הראשון של התרמודינמיקה.בתגובות כימיות הכוללת גזים ומתרחשות בלחץ האטמוספרה, העבודה הנעשית היא העבודה המכנית הקשורה לשינויי נפח התרחבות או התכווצות. לכן העבודה שווה לערך השלילי של הלחץ כפול השינוי בנפח. הצבת W בחוק הראשון של התרמודינמיקה וסידור מחדש של המשתנים במשוואה מראה ש-Q שווה לΔE ועוד P כפול ΔV, ומתקבל הביטוי של העברת חום בלחץ קבוע.בתגובות כימיות אחרות כמו בערה של עץ לצורך בישול מזון, יותר רלוונטי לכמת את החום שנפלט לצורך הבישול מאשר למדוד את כמות עבודת ההתפשטות שנעשית על הסביבה. מאחר שאנרגיה פנימית מתייחסת גם לחום וגם לעבודה, ΔE לא משמשת בתנאי לחץ קבוע. כדי לדון באופן בלעדי במעבר האנרגיה בצורת חום, מוגדרת צורה חדשה של תרמודינמיקה אנתלפיה.אנתלפיה, H, שווה לסכום האנרגיה הפנימית E, ועבדות הלחץ נפח, PV.מכיוון שאנרגיה, לחץ ונפח הן פונקציות מצב, גם אנתלפיה היא פונקצית מצב. ערכי אנתלפיה מוחלטים של חומרים ספציפיים לא ניתנים למדידה. ניתן לקבוע רק את השינוי באנתלפיה.שינוי באנתלפיה, ΔH, שווה לשינוי באנרגיה הפנימית, ΔE, ועוד P כפול ΔV.נזכור שהשינוי באנרגיה הוא סכום החום ועוד עבודת לחץ-נפח. ניתן לשלב את המשוואה כדי להראות שבתנאי לחץ קבוע דלתא H שווה לחום, Q, שהמערכת קיבלה או איבדה. אם המערכת מאבדת אנרגיה לסביבתה בצורה של חום, כמו במקרה של העץ הבוער, הטמפרטורה של הסביבה עולה.זה מתואר באמצעות סימן מינוס ל-Q. בהתאם לכך, ΔH הופך לשלילי והתהליך מתואר כאקסותרמי. לעומת זאת, אם מערכת מקבלת אנרגיה מהסביבה בצורה של חום כמו בתגובה המתרחשת בשימוש בשקית קירור כימית, הטמפרטורה של הסביבה יורדת.החום, במקרה הזה, מתואר באמצעות סימן חיובי. זה הופך את ΔH לחיובית והתהליך נקרא אנדותרמי.

<ol>
	<li>Canagaratna, סבסטיאן ג '"סיוע חזותי בחישובי אנתלפיה". כתב עת לחינוך כימי 77, מס '9 (2000): 1178.</li>
	<li>הווארד, אירמגארד ק. "H מיועד לאנתלפיה, הודות להייקה קמרלינג אונס ואלפרד ו. פורטר." כתב עת לחינוך כימי 79, מס '6 (2002): 697.</li>
	<li>ואן נס, הנדריק ג. תרמודינמיקה קלאסית של תמיסות שאינן אלקטרוליטים. Elsevier, 2015. 
	 </li>
</ol>

אנתלפיה

<div style="direction:rtl">

 כימאים משתמשים בדרך כלל בתכונה המכונה אנתלפיה (H) כדי לתאר את התרמודינמיקה של תהליכים כימיים ופיזיקליים. אנתלפיה מוגדרת כסכום האנרגיה הפנימית של המערכת (E) והמכפלה המתמטית של הלחץ (P) והנפח שלה (V): 
 <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/796/796_Equations-01.png" style="height: 40px;"> 

 אנתלפיה היא פונקציית מצב. לא ניתן למדוד באופן ישיר ערכי אנתלפיה עבור חומרים ספציפיים; ניתן לקבוע רק שינויים באנתלפיה עבור תהליכים כימיים או פיזיקליים. עבור תהליכים המתרחשים בלחץ קבוע (מצב שכיח לשינויים כימיים ופיזיקליים רבים), שינוי האנתלפיה (ΔH) הוא: 
 <img alt="Eq2" src="https://www.jove.com/files/core/CDNSource/lessons/796/796_Equations-02.png" style="height: 40px;"> 

 התוצאה המתמטית PΔV מייצגת עבודה (w), כלומר, התפשטות או עבודת לחץ-נפח. לפי ההגדרות שלהם, הסימנים האריתמטיים של ΔV ו-w יהיו תמיד הפוכים:
 <img alt="Eq3" src="https://www.jove.com/files/core/CDNSource/lessons/796/796_Equations-03.png" style="height: 40px;"> 

 החלפת המשוואה הזו וההגדרה של אנרגיה פנימית בלחץ קבוע (ΔE = qp + w) במשוואת שינוי האנתלפיה מניבה: 
 <img alt="Eq4" src="https://www.jove.com/files/core/CDNSource/lessons/796/796_Equations-04.png" style="height: 40px;"> 

 כאשר qp הוא חום התגובה בתנאי לחץ קבוע. 

 וכך, אם תהליך כימי או פיזיקלי מתבצע בלחץ קבוע כשהעבודה היחידה שנעשתה כתוצאה מהתפשטות או התכווצות (עבודה P-V), זרימת החום (qp) ושינוי האנתלפיה (ΔH) עבור התהליך שווים.

 החום המופק בזמן הפעלת מבער בונזן שווה לשינוי האנתלפיה של תגובת שריפת המתאן מאחר שהיא מתרחשת בלחץ הקבוע באטמוספירה. כימאים מבצעים בדרך כלל ניסויים בתנאים אטמוספריים רגילים, בלחץ חיצוני קבוע עם qp = ΔH, מה שהופך את האנתלפיה לבחירה הנוחה ביותר לקביעת שינויי חום לתגובות כימיות. 

 ערך שלילי של שינוי אנתלפיה, ΔH < 0, מצביע על תגובה אקסותרמית (חום המופק לסביבה); ערך חיובי, ΔH > 0, מצביע על תגובה אנדותרמית (חום שנספג מהסביבה). אם הכיוון של משוואה כימית מתהפך, הסימן האריתמטי של ה-ΔH שלה משתנה (תהליך שהוא אנדותרמי בכיוון אחד או אקסותרמי בכיוון ההפוך). 

 מבחינה מושגית, ΔE (מדד של חום ועבודה) ו-ΔH (מדד של חום בלחץ קבוע) שניהם מייצגים שינויים בפונקציית המצב עבור המערכת. בתהליכים שבהם השינוי בנפח, ΔV, קטן (המסת קרח), ו-ΔE ו-ΔH זהים. עם זאת, אם השינוי בנפח משמעותי (אידוי מים), כמות האנרגיה המועברת כעבודה תהיה משמעותית; לפיכך, ל- ΔE ו- ΔH יש ערכים שונים באופן משמעותי.

 טקסט זה מותאם מ <a href="https://openstax.org/books/chemistry-2e/pages/5-3-enthalpy">Openstax, Chemistry 2e, Section 5.3: Enthalpy</a>.</div>

כימאים משתמשים בדרך כלל בתכונה הידועה בשם אנתלפיה (H) כדי לתאר את התרמודינמיקה של תהליכים כימיים ופיזיקליים. אנתלפיה מוגדרת כסכום ...

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enthalpy and heat at constant pressure

Enthalpy describes heat changes in chemical and physical processes. Chemists use the symbol H for enthalpy. It is defined as a system’s internal energy, E, plus the product of pressure, P, and volume, V. Enthalpy is a state function, so only changes in enthalpy can be measured, not the enthalpy of a substance by itself.

For many reactions, the pressure stays constant. Under those conditions, the enthalpy change, ΔH, can be written in a way that includes pressure-volume work. The term PΔV represents expansion work, also called pressure-volume work. The signs of ΔV and w are always opposite, because expansion and work use opposite sign conventions.

At constant pressure, the internal energy change is ΔE = qp + w, where qp is the heat of reaction. When the only work done is due to expansion or contraction, qp and ΔH are equal. This is why enthalpy is a useful choice for measuring heat changes in many lab reactions and physical changes. A Bunsen burner is one example, since methane combustion occurs at about atmospheric pressure.

A negative ΔH means the process is exothermic, which means heat is given off to the surroundings. A positive ΔH means the process is endothermic, which means heat is absorbed from the surroundings. If a chemical equation is reversed, the sign of ΔH also changes. A process that is endothermic in one direction becomes exothermic in the other.

Enthalpy change and internal energy change both describe changes in a state function for the system. When the volume change, ΔV, is small, such as during melting of ice, ΔE and ΔH are essentially the same. When the volume change is larger, such as during evaporation of water, more energy is transferred as work. In that case, ΔE and ΔH can differ by a significant amount.

Enthalpy and Heat at Constant Pressure

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The kinetic molecular theory qualitatively explains the behaviors described by the various gas laws. The postulates of this theory may be applied in a ...

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Behavior of Gas Molecules: Molecular Diffusion, Mean Free Path, and Effusion

Although gaseous molecules travel at tremendous speeds (hundreds of meters per second), they collide with other gaseous molecules and travel in many ...

real-gases-effects-intermolecular-forces-molecular-volume-deriving

Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation

Thus far, the ideal gas law, PV = nRT, has been applied to a variety of different types of problems, ranging from reaction stoichiometry and empirical and ...

Ideal Gas Law

Source: Laboratory of Dr. Andreas Z&#252;ttel - Swiss Federal Laboratories for Materials Science and Technology
The ideal gas law describes the behavior ...

Derivation of the Ideal Gas Law
Gases are a fundamental state of matter. A gas is a collection of molecules that have a significant distance between their ...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Preparation of the LaboratoryExpand
	Here, we show the laboratory preparation for 10 students ...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Determining the Mass of the Unknown LiquidExpand
	According to the ideal gas law for a given ...

Use mathematics and computational thinking to explain the relationships among pressure, temperature, volume, and quantity of gas, both qualitatively and quantitatively.

PS.Chm.7.3

Understand the relationship among pressure, temperature, volume, and phase.

Enthalpy and Heat at Constant Pressure

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