Figure 11.12 uses squares to represent Element M and circles to represent Element N. a. Write th

step 1 Okay, so this problem is a little exercise in stoichiometry. And this is referring to in chemist

Figure 11.12 uses squares to represent Element M and circles...

Key Concepts

Balanced Chemical Equations

A balanced chemical equation shows the conservation of mass by ensuring that the number of atoms for each element is the same on both sides of the reaction. It provides the stoichiometric coefficients that indicate the relative proportions of reactants and products involved in the reaction.

Mole Concept

The mole is a fundamental unit in chemistry that quantifies the amount of substance. It provides a bridge between the atomic scale and the macroscopic scale, allowing chemists to count particles by using quantities expressed in moles. This concept is critical in converting between the number of particles and measurable quantities like mass.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It relies on the mole ratios derived from a balanced equation to calculate the amounts of substances consumed and produced, hence forming the basis for reaction yield predictions.

Limiting and Excess Reactants

In a chemical reaction, the limiting reactant is the reactant that is completely consumed, thereby limiting the extent of the reaction and determining the amount of product formed. The excess reactant is the one that remains unreacted after the completion of the reaction. Identifying these reactants is essential for predicting how much product will form and for optimizing the use of resources.

Transcript

00:01 Okay, so this problem is a little exercise in stoichiometry.

00:03 And this is referring to in chemistry when you have an equation, you want to balance it to make sure you have an equal amount of each element on every side.

00:12 And you see what is actually happening, sorry, to each atom or each element that is a part of this reaction.

00:19 So in this exercise, we're given a diagram here on the left.

00:23 And instead of looking at atoms, we're looking at blocks and circles or squares and circles, which are labeled.

00:30 To be m as the squares and then circles as the n so we need to work through this problem as if they are normal atoms and it's a great exercise to make sure we understand the concepts so the first part is to write a balanced equation for the reaction so to do this we need to see what we're looking at on both sides and was actually taking place in the reaction right so on the left we have our ms and our ns and we see that they are existing in pairs.

01:01 So kind of like a diatomic that you witness as h2 or o2, respectively being in their gas forms.

01:10 So part a, we see on the reactant side, we have m2.

01:17 I'll write this below.

01:18 We have m2 plus n2.

01:27 And then we don't know if this reaction is reversible or not.

01:29 So let's go over to the product side.

01:33 So i just drew a street arrow rather than a reversible reaction.

01:35 So one of the products we see formed is this new structure here where we see three blocks, three squares in one circle.

01:48 So that would lead us to believe there's three ms and one n.

01:51 So we should write it out as m3n because that's what is existing as a molecule.

01:58 And then we have some n2.

02:04 So it doesn't look like we formed anything new here, but we still have some n2 on the product side.

02:09 So let's count everything to make sure that it's balanced.

02:14 So i see over here we have 2 and 2 for m and n.

02:23 I'll write it in the respective colors so it's easy to see.

02:27 So 2 and 2.

02:30 Now on the right we see 3m because there's a 3 subscripted right next to it.

02:36 So 3 and then we see 1, 2, 3 ends.

02:42 So we can tell that things are not balanced.

02:46 So what common number can we get with ms? that's the smallest.

02:50 So two and three can both be multiplied to make six relatively easily.

02:55 Two times three is six.

02:57 Three times two is six.

02:59 So i'll put a three here.

03:03 Beautiful.

03:03 And i'll put two here.

03:08 Wonderful.

03:08 So now we have six m's.

03:10 But now we have four ends here, right? because two times one is two.

03:16 2, plus 2.

03:18 So we have 4 ends here and here.

03:23 So to make this a 4 here, just throw a 2.

03:26 Now we're balanced.

03:29 Yay! the first part is over.

03:32 So now we can move on to part b, where we are asked to count the moles of the reactants.

03:41 And we're told that you can consider each square to represent one mole of m and one circle represents one mole of n.

03:47 So just count the circles and the squares.

03:50 They're in pairs of two and there's three pairs of two.

03:53 So let's do this in blue.

03:55 There's six moles of m and also six moles of n...

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