.. _sphx_glr_api_gallery_analytical_stoichiometry:

Stoichiometry and elemental analysis
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Balancing chemical equations, limiting reagents and yields, and
empirical formulas from combustion-analysis data.


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    <div class="sphx-glr-thumbnails">

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    <div class="sphx-glr-thumbcontainer" tooltip="Jeremias Richter, who coined the word stoichiometry, tabulated how many parts by weight of each base neutralize a fixed weight of an acid, and found the proportions were fixed and mutually consistent. Today those numbers follow from a balanced equation and molar masses. balance_equation finds the smallest integer coefficients that conserve every element (and charge) as the exact null space of the composition matrix. Left: Richter-style neutralization equivalents, the grams of each base that neutralize 1000 g of sulfuric acid. Right: product yield as the N2:H2 feed ratio varies. It rises while H2 is limiting and falls once N2 is, with the kink at the stoichiometric 1:3 ratio (~chemistrykit.stoichiometry.limiting_reagent).">

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  .. image:: /api/gallery/analytical/stoichiometry/images/thumb/sphx_glr_plot_01_richter_stoichiometry_thumb.png
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  :doc:`/api/gallery/analytical/stoichiometry/plot_01_richter_stoichiometry`

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      <div class="sphx-glr-thumbnail-title">Richter's stoichiometry: equivalent weights, balanced equations, limiting reagents</div>
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    <div class="sphx-glr-thumbcontainer" tooltip="Justus von Liebig&#x27;s Kaliapparat made organic elemental analysis routine. The sample is burned in oxygen over hot copper oxide, the water is caught in calcium chloride, the CO2 in potash bulbs, and both are weighed. Carbon and hydrogen follow from those two masses, oxygen by difference. Below, a 10.00 mg sample of ascorbic acid (vitamin C) is &quot;burned&quot;. Its mass percentages go to empirical_formula, which converts to moles, divides by the smallest, and searches for the smallest multiplier that gives whole numbers. Here that gives C3H4O3, and a molar mass of about 176 g/mol then fixes the molecular formula as C6H8O6. The right panel shows why the multiplier search is needed: the raw mole ratios are 1 : 1.33 : 1, which become whole only after multiplying by 3.">

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  .. image:: /api/gallery/analytical/stoichiometry/images/thumb/sphx_glr_plot_02_liebig_combustion_analysis_thumb.png
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  :doc:`/api/gallery/analytical/stoichiometry/plot_02_liebig_combustion_analysis`

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      <div class="sphx-glr-thumbnail-title">Liebig's combustion analysis: an empirical formula from CO2 and H2O masses</div>
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    </div>


.. toctree::
   :hidden:

   /api/gallery/analytical/stoichiometry/plot_01_richter_stoichiometry
   /api/gallery/analytical/stoichiometry/plot_02_liebig_combustion_analysis