Consider the balanced chemical equation: A 2 + 2 B 2 → 2 AB 2 . A reaction is performed with the initial amounts of A 2 and B 2 shown in part (a). The amount of product obtained is shown in part (b). Calculate the percent yield. a. <IMAGE> b. <IMAGE>

Welcome back everyone. The reactant below combined. According to the following equation where M two reacts with three moles of X two to form two moles of MX three, the initial amounts of M two and X two are shown in figure A where are gray molecules are our and molecules and our orange molecules are our X molecules. While the actual yield is shown in figure B, what is the percent yield of the reaction? So counting our molds of our reactant, we can count seven moles of our M two di atomic molecule and 15 moles of our ex to die atomic molecule. For figure B, we can count a total of seven moles of our M X three product as our actual yield. We're going to begin by calculating the theoretical yield of MX three from each reactant. So beginning with our MX three from our first reactant em too, we're going to begin with our seven molecules of M two multiplied by the ratio between molecules of M two and our denominator. And I'll use shorthand for that word, two molecules of MX three. In our numerator, we are going to refer to our given equation in the prompt where we see that we have for one molecule of M two reacted to molecules of MX three produced. So canceling out molecules of em to our reactant. We're left with molecules of our product MX three. And this is going to result in a value of molecules Of MX three that is formed from this first reactant. Now, we need to compare our theoretical yields of MX three from our second reactant X two. So we have 15 molecules of X two in which we want to multiply by the conversion factor to go from molecules of X two in the denominator two molecules of our product MX three in the numerator. Again, referring to our bounced equation given in the prompt, we have three molecules of X two reacted for every two molecules of MX three produced. So three molecules of X two and the dominator 22 molecules of MX three in the numerator canceling out molecules of X two were left with molecules of MX three. And this is going to result in three or sorry, rather 10 molecules of our product MX three that is formed from our second reactant. So we need to find the percent yield for our final answer. Recall that we can calculate percent yield By taking our actual yield divided by our theoretical yield times 100%. And so what we'll find is that our actual yield given from figure being our prompt, we determined was seven molecules of our product. So seven molecules of MX three in our numerator for the actual yield. And in our denominator are theoretical yield is going to be the reactant that produced the lower amount of our product, which is our limiting reactant. And because we have only 10 molecules of MX three formed from X two, that means that X two is our limiting reactant and our molecules of MX three formed is our theoretical yield. So we would plug that in our denominator 10 molecules of MX three as our theoretical yield. Now multiplying this quotient by 100%, we're going to come up with our percent yield. which in the next line is equal to a value of 70%. And this would be our final answer as our percent yield for the reaction producing MX three, the product which corresponds to choice, seeing the multiple choice as the correct answer. So I hope everything I went through is clear and let us know if you have any questions.

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6. Chemical Reactions & Quantities

Percent Yield

GOB Chemistry

6. Chemical Reactions & Quantities

Percent Yield

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Problem 18

Textbook Question

Consider the balanced chemical equation: A₂ + 2 B₂ → 2 AB₂. A reaction is performed with the initial amounts of A₂ and B₂ shown in part (a). The amount of product obtained is shown in part (b). Calculate the percent yield.
a. <IMAGE>
b. <IMAGE>

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Step 1: Analyze the balanced chemical equation provided: A₂ + 2B₂ → 2AB₂. This equation indicates that one molecule of A₂ reacts with two molecules of B₂ to produce two molecules of AB₂.

Step 2: Count the initial number of molecules of A₂ and B₂ from the image labeled 'a'. There are 8 A₂ molecules and 16 B₂ molecules. These are the reactants available for the reaction.

Step 3: Determine the limiting reactant. Using the stoichiometric ratio from the balanced equation, 1 molecule of A₂ requires 2 molecules of B₂. Since there are 8 A₂ molecules, they would require 16 B₂ molecules to completely react. Both reactants are present in the exact stoichiometric ratio, so neither is in excess.

Step 4: Calculate the theoretical yield of AB₂. According to the balanced equation, 1 A₂ molecule produces 2 AB₂ molecules. Therefore, 8 A₂ molecules would theoretically produce 16 AB₂ molecules.

Step 5: Count the actual number of AB₂ molecules produced from the image labeled 'b'. There are 12 AB₂ molecules. Use the formula for percent yield: Percent Yield = (Actual Yield / Theoretical Yield) × 100. Substitute the values into the formula to calculate the percent yield.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a given reaction based on the balanced chemical equation. Understanding stoichiometry is essential for calculating theoretical yields and determining how much of each reactant is needed.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of a product obtained from the reaction to the theoretical yield predicted by stoichiometry. It is expressed as a percentage and is calculated using the formula: (actual yield / theoretical yield) × 100%. A high percent yield indicates a successful reaction, while a low percent yield may suggest incomplete reactions or losses during the process.

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction where the number of atoms for each element is the same on both sides of the equation. This balance ensures the law of conservation of mass is upheld, meaning matter is neither created nor destroyed in a chemical reaction. The coefficients in the equation indicate the ratios of reactants and products, which are crucial for stoichiometric calculations and determining yields.

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Consider the balanced chemical equation: A2 + 2 B2 → 2 AB2. A reaction is performed with the initial amounts of A2 and B2 shown in part (a). The amount of product obtained is shown in part (b). Calculate the percent yield. a. <IMAGE>b. <IMAGE>

Key Concepts

Stoichiometry

Percent Yield

Balanced Chemical Equation

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Consider the balanced chemical equation: A₂ + 2 B₂ → 2 AB₂. A reaction is performed with the initial amounts of A₂ and B₂ shown in part (a). The amount of product obtained is shown in part (b). Calculate the percent yield.
a. <IMAGE>
b. <IMAGE>