How To Solve Stoichiometry Problems Step By Step

How To Solve Stoichiometry Problems Step By Step-37
Below we will provide the most common and important conversion factors to convert between moles and grams, moles and volumes of gases, moles and molecules, and moles and solutions.These conversion factors function in the same way as those discussed in the previous section Note also that though these conversion factors focus on converting from some other unit to moles, they can also be turned around, allowing you to convert from moles to some other unit.So lets first figure out how many moles 85 grams are. So let me go down and figure out the atomic masses of iron and oxygen. But let's just say that the aluminium that we're dealing with has a mass of 27 atomic mass units. So if we need 1.06 moles, how many is that going to be? And if we had more than 28.62 grams of aluminium, then they'll be left over after this reaction happens.

Below we will provide the most common and important conversion factors to convert between moles and grams, moles and volumes of gases, moles and molecules, and moles and solutions.These conversion factors function in the same way as those discussed in the previous section Note also that though these conversion factors focus on converting from some other unit to moles, they can also be turned around, allowing you to convert from moles to some other unit.So lets first figure out how many moles 85 grams are. So let me go down and figure out the atomic masses of iron and oxygen. But let's just say that the aluminium that we're dealing with has a mass of 27 atomic mass units. So if we need 1.06 moles, how many is that going to be? And if we had more than 28.62 grams of aluminium, then they'll be left over after this reaction happens.

H2 Ca(Cl O3)2 This shows that for every 2 moles of chloric acid, 1 mol of hydrogen forms.

Thus, 0.207 moles chloric acid leads to 0.207/2 = 0.1036 moles hydrogen.

So it's a relationship between the reactants and the products in a balanced chemical equation. Just so we get practice balancing equations, I'm always going to start with unbalanced equations. How many iron atoms do we have on the right hand side? And then we need to have twice as many moles of aluminum. This mass is going to be 2 times 56 plus 3 times 16. But this isn't a math video, so I'll get the calculator out. So in our reaction we said we're starting off with 85 grams of iron oxide. Well 85 grams of iron three oxide is equal to 85 over 160 moles. So we're going to need 1.06 moles of aluminum. So for every mole of this, we need two moles of this.

So if we're given an unbalanced one, we know how to get to the balanced point. Because for every mole of the iron three oxide, we have two moles of aluminum. So that's equal to, 85 divided by 160 equals 0.53125. So everything we've done so far in this green and light blue, we figured out how many moles 85 grams of iron three oxide is. If we have 0.53 moles, you multiply that by 2, and you have 1.06 moles of aluminum.

Stoichiometric calculations are based on the equalization between the ratio of the amount of substance we're interested in, and the ratio of the corresponding absolute values of the stoichiometric numbers. As before, the path to the solution begins with the first (and hardest) step, which requires of you to not only keep your eyes sharp, but also your mind.

Almost every single stoichiometric task can be solved in five easy steps, and with only a basic knowledge of mathematics. Before you even begin, make sure to carefully read the task itself.The constituent parts of a chemical equation are never destroyed or lost: the yield of a reaction must exactly correspond to the original reagents.This fact holds not just for the type of elements in the yield, but also the number.Stoichiometry is the measure of the elements within a reaction.It involves calculations that take into account the masses of reactants and products in a given chemical reaction.But it's really just the study or the calculation of the relationships between the different molecules in a reaction. Or if I give you y grams of this molecule and z grams of this molecule which one's going to run out first? And we'll actually do those exact two types of problems in this video.This is the actual definition that Wikipedia gives, stoichiometry is the calculation of quantitative, or measurable, relationships of the reactants and the products. So let's say that we were given 85 grams of the iron three oxide.Now, we're ready to learn about stoichiometry.And this is an ultra fancy word that often makes people think it's difficult. There's not just one type of stoichiometry problem, but they're all along the lines of, if I give you x grams of this how many grams of aluminum do I need to make this reaction happen?And you're going to see in chemistry, sometimes people use the word reagents. Aluminum, on the left hand side we only have one aluminum atom. So my question to you is how many grams of aluminum do we need?For most of our purposes you can use the word reagents and reactants interchangeably. The reagents are sometimes for special types of reactions where you want to throw a reagent in and see if something happens. So remember when we're doing stoichiometry first of all, we want to deal with balanced equations. Well you look at the equation, you immediately see the mole ratio.

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