You see, the conversions from liters to moles and back to liters are the same for both gases, so the only number that really mattered, in this case, was the mole ratio between the reactant and the product (in other words, the fact that it took two . Well, first of all, it’s good practice to do it the long way, and it helps to understand the fundamentals.
And on the AP Chemistry exam, it’s often worth the extra two minutes to write out your entire thought process on a stoichiometry problem, especially if it’s a long answer.
However, if this seems obvious to you, keep it in mind; it may come in handy at some point.
Titration may seem like an intimidating topic, but while it is a little involved, it simply builds on the concepts we already know from expected values and limiting reactants. A little explanation: titration is basically just adding one compound to another in solution (in this case, adding a base to an acid) and seeing how the p H changes. Those are the five main applications of stoichiometry on the AP Chemistry exam.
This balanced equation tells us a lot about how this reaction works. This one is another very important application of stoichiometry for the AP Chemistry exam.
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The core concept we can take away from it is that one molecule of methane combines with two molecules of diatomic oxygen to form one molecule of carbon dioxide and two molecules of water, or correspondingly, that one mole of methane combines with two moles of diatomic oxygen to form one mole of carbon dioxide and two moles of water. A note about nomenclature: saying reagent makes me feel like a mysterious alchemist, but I’m going to favor reactant because I think it’s a little bit clearer.Let’s say that we have this equation, which is the combustion of methane. Then I do the same on the right side: one carbon, two hydrogens, and three oxygens. The only way to get that four hydrogens is to double the amount of …and this equation is now balanced.You’ve probably learned much of this even in a non-AP chemistry class, so bear with me; it’ll get more advanced.Percent yield is a way of quantifying the difference between the theoretical yield (the expected value) and the experimental yield.Using the same reaction yet again, let’s say that you were given a problem like this. In fact, there is an easier way to do this calculation.This concept is very important to the applications of stoichiometry. For the sake of simplicity, we’re going to continue to use the combustion of methane as our reaction in question. We have more moles of oxygen, so methane is the limiting reactant, right?No, because in the reaction, we can see that we need twice as many moles of oxygen as of methane.That being said, if you’re pressed for time, you can try it.Recall this question: , meaning that we need twice as many moles of oxygen as we do methane.The AACT high school classroom resource library has everything you need to put together a unit plan for your classroom: lessons, activities, labs, projects, videos, simulations, and animations.We constructed a unit plan using AACT resources that is designed to teach the concepts of stoichiometry and limiting reactants to your students.