Consider the following reaction:
I2O5 (g) + 5 CO (g) --> 5 CO2 (g) + I2
(a) 80.0 grams of Iodine (V) oxide reacts with 28.0 grams of carbon monoxide. Determine the mass of iodine which could be produced.
(b) If only 0.160 moles of Iodine was produced in part (a), what percentage yield of iodine was produced?
Limiting Reactant Problem
As a chemical reaction occurs, the reactants will continue to produce product as long as the correct conditions for the reaction are present and all reactants are available. Once one of the reactants is used up, the reaction stops. The reactant that is used up first is called the limiting reactant because it limits the amount of product that can be made. The other reactant(s) tends to be in excess, meaning a greater relative amount of it exists the limiting reactant. We call it the excess reactant. It's just like when you go to make cookies, you may have all the flour, butter and oil that you need but without any eggs you cannot make them. In this example, the flour butter and oil are in excess where the eggs limit the product.
Answer and Explanation:
a. This is a limiting reactant problem and first we must decide which reactant limits the process. This is done by comparing the relative amounts of...
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from Chemistry 101: General ChemistryChapter 9 / Lesson 5