12: Stoichiometry
- Page ID
- 53788
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 12.1: Everyday Stoichiometry
- This page explores stoichiometry through a practical ham sandwich example, detailing how to calculate ingredient requirements using balanced equations. It highlights the role of stoichiometry in determining reactant quantities and includes a problem-solving exercise for calculating pickles needed based on available ham slices. The text encourages reader engagement by introducing a smoothie-related example to further illustrate stoichiometric principles.
- 12.2: Mole Ratios
- This page covers mole ratios in stoichiometry, detailing how they connect the amounts of substances in chemical reactions through balanced equations, particularly the Haber process. It highlights the utility of mole ratios in predicting product quantities while adhering to the conservation of mass. Additionally, the text includes a problem-solving example for calculating ammonia production from a specified amount of hydrogen.
- 12.3: Mass-Mole Stoichiometry
- This page covers mass-mole stoichiometry, focusing on mole-mass conversions essential for chemical calculations in large construction projects. It explains resolving mass-to-moles and moles-to-mass problems using balanced equations and molar mass, illustrated with examples like reactions involving hydrogen fluoride and sulfur dioxide. Key points include the necessity of a balanced equation and attention to significant figures in calculations.
- 12.4: Mass-Mass Stoichiometry
- This page explains mass-mass stoichiometry calculations, highlighting the conversion of substance mass to moles and then to product mass via a chemical equation. It includes an example of ammonium nitrate decomposition into dinitrogen monoxide and water, detailing the necessary calculation steps. The text emphasizes the law of conservation of mass and the importance of accurate chemical formulas, serving as a guide for performing these calculations in chemistry.
- 12.5: Volume-Volume Stoichiometry
- This page discusses propane grills and methods to gauge propane levels using pressure gauges. It introduces volume-volume stoichiometry based on Avogadro's hypothesis, explaining that equal gas volumes at the same temperature and pressure contain the same particle number.
- 12.6: Mass-Volume Stoichiometry
- This page discusses stoichiometry in chemical reactions, highlighting the use of sodium azide in air bags for nitrogen gas production. It presents mass-volume and volume-mass problems, providing examples such as calculating hydrogen gas volume from aluminum and sulfuric acid reactions, and determining calcium oxide mass for reacting with sulfur dioxide. The importance of accurate ratios and unit conversions in these calculations is emphasized.
- 12.7: Limiting Reactant
- This page explains limiting reactants in chemistry through a cooking analogy and the Haber process. It compares the need for specific ingredient ratios in cooking to the requirements in chemical reactions. In the Haber process, hydrogen is the limiting reactant, fully consumed before nitrogen, which remains in excess. The text includes review questions for reinforcing understanding of these concepts.
- 12.8: Determining the Limiting Reactant
- This page explains how to find the limiting reactant in a chemical reaction, illustrated by the reaction of silver and sulfur to form silver sulfide. It details steps to convert mass to moles, use a balanced equation for mole ratios, and identify excess reactants. In the example provided, silver is the limiting reactant, while sulfur remains in excess. Additionally, it outlines how to calculate the mass of the excess reactant left after the reaction.
- 12.9: Theoretical Yield and Percent Yield
- This page discusses the complexities and costs of pharmaceutical production, emphasizing the importance of improving drug synthesis efficiency. It highlights percent yield, the ratio of actual to theoretical yield, as a key metric for assessing chemical reaction success. Factors such as incomplete reactions and impurities often result in yields below 100%. Achieving higher percent yields is essential for minimizing waste and reducing costs in drug manufacturing.