Examine the reaction represented in Figure 11.14 . Determine if the reaction went to completion.

Examine the reaction represented in Figure 11.14 . Determine...

Key Concepts

Reaction Completion

This concept involves determining whether a chemical reaction proceeds until all of one or more reactants have been completely converted into products. Understanding reaction completion is key to analyzing if a reaction has reached its maximum extent or if it stops at an equilibrium point with some reactants remaining.

Percent Yield

Percent yield quantifies the efficiency of a reaction by comparing the actual amount of product obtained to the theoretical amount predicted by stoichiometric calculations. It is calculated by dividing the actual yield by the theoretical yield and then multiplying by 100, providing insight into losses or side reactions that may occur during the process.

Stoichiometry

Stoichiometry deals with the quantitative relationships between reactants and products in a balanced chemical equation. It is essential for calculating the theoretical yield of a reaction and understanding how the amounts of various substances relate to one another during a chemical transformation.

Limiting Reactant

The limiting reactant is the substance in a reaction that is completely consumed first, thereby limiting the amount of product that can be formed. Identifying the limiting reactant is critical for determining the theoretical yield and assessing whether the reaction has gone to completion.

Transcript

00:01 In this question, we need to determine whether the reaction that is represented in the figure went to completion.

00:09 In order to do that, we need to first represent with a balanced chemical equation what is going on in the figure.

00:20 What we are seeing is that, and based on the symbols, what we are seeing is that eight moles of a, substance a, are mixed together with eight moles of substance b and after the reaction takes place, we end up with three moles of the compound ab2, five moles of a, of substance a and two moles of substance b.

00:59 So this is what is going on.

01:02 This equation represents the figure that is displayed.

01:08 Therefore, what we have, if we know that we have an excess of five moles of a, then only three moles of a reacted.

01:23 If we have an excess of two moles of b, then we know that six moles of b reacted.

01:34 To produce three moles of ab2.

01:40 The balanced chemical equation using the minimum whole numbers is obtained when we divide this equation by three and then we have a reacting with 2b to produce one more of ab2.

02:02 So one more of a reacts with two modes of b to produce one more of ab2.

02:07 This is the balanced equation for the reaction that is going on.

02:15 So the question is whether the reaction went to completion.

02:21 Because we have eight moles of a, big mix with eight moles of b, and the ratio is one mole of a should react.

02:42 With two moles of b, we can say that the reaction did not go to completion.

02:53 Because you have excess of both a and b, and we're going to see that when we determine which one is the limiting reagent here.

03:06 To determine the limiting reagent, we won't establish the theoretical ratio.

03:10 The theoretical ratio is 1 mole of a to 2 moles of b.

03:19 And this number is 0 .5, this ratio.

03:24 And now we are going to compare this theoretical ratio with the experimental ratio or actual ratio, which is 8 moles of a being mixed with 8 moles of b.

03:40 And this ratio is 1.

03:43 Therefore, the theoretical ratio is less than the experimental ratio...

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