# How To Solve Mass To Mass Stoichiometry Problems

Composition stoichiometry describes the quantitative relationships among elements in compounds.It can be used to determine the number of atoms present in a collection of molecules and the masses of each.

Composition stoichiometry describes the quantitative relationships among elements in compounds.It can be used to determine the number of atoms present in a collection of molecules and the masses of each.

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Sadly, for this example, we have to move on from our beloved methane combustion equation ( Pretty intimidating if you don’t know what to do, right? In this case, we can see that the p H passes through the equivalence point (where the acid and the base cancel each other out and the p H is of oxalic acid. You’ll notice that the common thread running through all of them is the expected value.

Essentially, if you understand expected value really well, you should be able to figure out most of the rest.

Solving Mass-Mass Stoichiometry Problems: German chemist Jeremias Benjaim Richter was the first to lay down the principles of stoichiometry in 1792.

Richter discovered that the ratio by weight of the compounds consumed in a chemical reaction was always the same.

In other words, stoichiometry is the practice of using a chemical reaction equation to predict the results of the reaction. Of course, that means that we need to start with a chemical reaction.

When we look at the two sides of the reaction, we have to make sure that the number of atoms of each element on each side is the same because of the principle of conservation of mass. In this section of the AP Chemistry Crash Course, we’ll start by looking at the basic concepts of stoichiometry, and then we’ll cover five applications for 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.

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.