Understanding Limiting Reactants

Therefore no more casseroles can be made in this

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flour, and milk will remain, but all the green chiles will be used. Therefore, no more casseroles can be made. In this example, the green chiles are the limiting reactant . The limiting reactant is the reactant that is consumed first and limits the amount of product that can be made. The same principle applies in determining the quantity of product that can be produced in a chemical reaction. Let’s take another look at the reaction of hydrogen and oxygen to produce water, then consider what would happen if 2.00 mol hydrogen and 2.00 mol oxygen were available. How many moles of water can be produced? What is the limiting reactant? Which reactant will be in excess and by how much? 2 H 2 (g) + O 2 (g) → 2 H 2 O(l) The balanced chemical equation states that 2.00 mol hydrogen react with 1.00 mol oxygen. When the reaction is complete, 2.00 mol water are produced and 1.00 mol oxygen remains unreacted. This problem is easy to solve by inspection. A more systematic way to solve the problem is to create an SRF table, as shown in Figure 24. The table is composed of the following lines: Line 1: The balanced chemical equation is listed. Line 2: The Starting number of moles of each substance is listed. This would be what is available, the same as the ingredients for the casseroles. Line 3: The Reacting ratio determined from the coefficients in the balanced equation is multiplied by x, the basic amount of moles that will react. The reactants are being consumed so a minus sign is placed in front of them. The products are increasing so a plus sign is placed in front
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  • Spring '13
  • Dr.Sharma
  • Stoichiometry, Chemical reaction, Reagent

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