Limiting Reactants

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The quantity exceeds the amount required by the reaction’s stoichiometry. This is done, to ensure that all of the other expensive reactant is completely used up in the chemical reaction. Sometimes, this strategy is employed to make reactions occur faster. For example, we know that a large quantity of oxygen in a chemical reaction makes things burn more rapidly. In this way, excess of oxygen is left behind at the end of reaction and the other reactant is consumed earlier. This reactant which is consumed earlier is called a limiting reactant.

Thermogravimetric analysis curves obtained in air for GAB, GAB-BBSs, GAB-M, and GAB-M–BBSs in ; weight and derivate weight curves of BBSs in . The values indicated in the figure represent the residual weight measured for the materials at 650°C; the vertical broken lines indicate the temperature of 200°C used for the quantification of water and organics loss. Nitrogen adsorption–desorption measurements at 77 K were carried out by means of ASAP 2020 Micromeritics gas-volumetric apparatus.

One mole of sulfuric acid makes one mole of copper sulfate (0.1 mol). Since one mole of iron reacts with one mole of sulfur, there is insufficient iron to react with all of the sulfur used in the experiment, therefore the iron is the limiting reactant. More examples of % yield and atom economy calculations in section 6. It would be normal to use excess of the copper oxide, because it is easy to separate by filtration the unreacted oxide to leave a neutral solution of the salt, so you would use more than the 16 g of CuO calculated in part 3. Again, I’ve set out the solution to the problem in the form of a ‘logic’ table not using moles.

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According to the equation each mole of Mg requires two moles of HCl to complete the reaction. Salt crystals you would filter off the excess copper oxide, so this is a viable recipe for making copper sulfate crystals.. In this case the metal is automatically the limiting if it is fully exposed to excess of air, effectively excess oxygen.