Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. Fe2 O3(s)+3 CO(g

step 1 Okay, so this problem has two parts. It has a part A and a part B. And this whole problem is bas

Iron(III) oxide reacts with carbon monoxide to produce iron...

Key Concepts

Balanced Chemical Equation

A balanced chemical equation shows the reactants and products in a chemical reaction with their corresponding stoichiometric coefficients. It ensures that matter is conserved by having the same number of atoms of each element on both sides. This forms the basis for quantitative calculations in chemical reactions.

Stoichiometry

Stoichiometry involves using the relationships expressed in a balanced chemical equation to calculate quantities, such as moles and masses, of reactants and products. It is the key tool for converting given amounts of substances to the required number of moles using molar masses and the mole ratios from the equation.

Molar Mass

Molar mass is the mass of one mole of a substance, usually expressed in grams per mole. It is used to convert between the mass of a substance and the number of moles, which is essential for applying the mole ratios from the balanced chemical equation to calculate theoretical yields.

Theoretical Yield

The theoretical yield is the maximum amount of product that can be formed from a given amount of reactant, assuming complete conversion and no losses. It is calculated using stoichiometry and molar masses, based on the proportions dictated by the balanced chemical equation.

Percent Yield

Percent yield compares the actual yield obtained in an experiment to the theoretical yield calculated by stoichiometry, and it is expressed as a percentage. It provides a measure of the efficiency of a chemical reaction and is calculated by dividing the actual yield by the theoretical yield and multiplying by 100.

Transcript

00:01 Okay, so this problem has two parts.

00:05 It has a part a and a part b.

00:07 And this whole problem is based on finding a theoretical yield.

00:12 So to find a theoretical yield, you're going to end up doing a gram -to -gram conversion of your limiting reactant or whatever reactant they say is limiting.

00:35 And that's going to give you in every, that's going to give you in the perfect world, in the perfect clean lab, where everything goes perfectly swell, how much you should produce.

00:48 Then you have actual yield, which will be provided to you in each problem, because this is how much was actually measured.

01:04 So scientists try to get an idea of this by taking actual, dividing it by theoretical, multiply it by 100, and that gives them something called percent yield.

01:21 So all these problems are about percent yield or both of these problems i should say are about percent yield.

01:28 We're going to have to find theoretical yield first and then we're going to have to find theoretical yield first and then we're going to have to convert or then do the percent yield math.

01:37 So part a gives us a mass of 65 .0 grams of fe203.

01:47 And it also tells us that 15 grams of fe were produced.

01:58 So then we know that we are trying to shoot towards fe.

02:03 So we're going to do a gram to gram with 65 grams of fe2 .3 and get it to grams of fe.

02:08 That's our first step.

02:10 So to do that, we're going to first do our three -step conversion.

02:28 Remember to get the molar mass, you have to look at the period.

02:31 Table.

02:33 So if you add iron times two plus oxygen times three, you end up getting a mass of 159 .7.

02:42 So blue is the periodic table.

02:47 So that gets us rid of, that gets us two moles from grams.

02:51 So now we have to get rid of these moles.

02:53 So we're going to put moles of f .e.

02:54 203 on the bottom.

02:56 And we're trying to get to grams of fe, but we can't go straight there.

02:59 So instead we're going to go moles of fe.

03:01 When we have moles on top of moles, we have to look at our balanced chemical reaction.

03:07 So if we look at fe, the coefficient is 2.

03:10 If we look at fe203, there is no coefficient, therefore it is 1.

03:16 The last step to finding the theoretical yield, we have to convert this moles of fe to grams of fe.

03:25 And we are going to do that by using the periodic table.

03:29 The mass of fe is 55 .85.

03:33 So when we calculate all of this out, we get a theoretical yield of 45 .5 grams.

03:42 So then the second part, now that we have our theoretical yield, we're going to take our actual yield, which is 15 .0, divided by that 45 .5 grams, and then we're going to multiply the whole thing by 100...

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