1: Introductory Remarks
- Page ID
- 7213
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 1.1: Introduction
- This page introduces the academic approach to thermodynamics, highlighting its crucial principles for engineering despite their abstract nature. It acknowledges the disconnect engineers might feel but asserts that these concepts are essential for practical applications. Initial chapters will cover relevant mathematical concepts like partial derivatives, with deeper thermodynamic discussions planned for later in the text.
- 1.2: Caloric, Calories, Heat and Energy
- This page examines the historical progression of heat as energy, moving from caloric theory to viewing heat as motion, influenced by scientists such as Davy and Thompson. It highlights Joule's experiments that established the mechanical equivalent of heat, connecting work to heat generation. Although joules are theoretically preferred for measuring heat, calories are still commonly used, especially in nutrition, complicating thermodynamic equations.
- 1.3: Extensive and Intensive Quantities
- This page explores the difference between extensive and intensive quantities in thermodynamics. It defines extensive quantities (e.g., heat capacity, volume) as dependent on material amount, while intensive quantities (e.g., temperature, pressure) are independent. Specific and molar heat capacities are noted as intensive examples.
- 1.4: Mole
- This page covers Avogadro's number (6.022 x 10^23), defining a mole as the quantity of substance containing this number of entities, including atoms and molecules. It highlights the historical choice of carbon-12 as a reference and introduces molar mass, noting that 28 grams of nitrogen gas aligns with its molecular weight. The use of the kilomole (10^3 moles) for SI calculations is also mentioned.
- 1.5: Prepositions
- This page underscores the importance of precise language regarding prepositions in thermodynamics. It stresses that numerical answers for heat and work must be accompanied by clear indicators of whether heat was gained or lost and if work was done on or by the gas. Ambiguities in these details can result in misunderstandings and marks lost in assessments. Students are encouraged to be specific to enhance clarity in their responses.
- 1.6: Applicability of Equations
- This page emphasizes the importance of understanding the applicability of equations in thermodynamics. It contrasts the universally applicable First Law of Thermodynamics with the more limited equation for ideal gases, noting that the latter does not apply to all states of matter. The key takeaway is the necessity for caution in using these equations, highlighting the need to recognize their specific conditions and limitations.