If blue spheres represent nitrogen atoms and purple spheres...

If blue spheres represent nitrogen atoms and purple spheres represent iodine atoms, $(7.1,7.8)$
a. Write a balanced equation for the reaction.
b. from the diagram of the actual products that result, calculate the percent yield for the reaction.

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Key Concepts

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. By using the mole ratios derived from a balanced chemical equation, one can calculate the amounts of substances consumed or produced during the reaction.

Percent Yield

Percent yield is a quantitative measure that compares the actual yield of a product obtained from an experiment to the theoretical yield predicted by stoichiometry. It is calculated using the formula: (actual yield/theoretical yield) x 100%, and provides insight into the efficiency and practical limitations of a chemical reaction.

Balanced Chemical Equation

A balanced chemical equation represents a reaction in which the number of atoms for each element is the same on both the reactants and products sides, reflecting the law of conservation of mass. The equation uses coefficients that indicate the relative proportions of each substance involved in the reaction.

Transcript

00:01 This question has two parts.

00:02 So the first part is asking us to write a balance equation for the reaction.

00:06 So let's take a look.

00:07 What kinds of reactants do we have? well, our reactants are going to be these molecules consisting of four atoms.

00:15 Three of those atoms are purple.

00:17 So those are iodines.

00:19 And then the other one atom is blue, so it's a nitrogen.

00:24 So we would write this as n -i -3.

00:29 Nitrogen tri -iodide.

00:33 And what about our products? well, we see that with our products, we form both diatomic blue, so n2, and we form diatomic purple, which is i2.

00:50 So let's write our equation.

00:54 N i3 produces n2 plus i2.

01:02 So how do we balance this? well, we can see that there's three iodins on the left.

01:08 There's two on the right.

01:09 So what we can do is we can find the, um, greatest common factor essentially, right? so we're going to put a two out here.

01:18 So that'll make this a total of six iodines, right? and on the right, we're going to put a three out here because that'll make it another total of six iodines.

01:29 So now this is balanced, right? there's six on both sides.

01:32 What about our nitrogens? well, there's two nitrogens on the left...

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