/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 33 What is the theoretical yield fo... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 5: Problem 33

What is the theoretical yield for a reaction, and how does this quantity depend on the limiting reactant?

Short Answer

Expert verified
The theoretical yield is the maximum amount of product that can be formed in a chemical reaction based on the stoichiometric ratios of the reactants in the balanced chemical equation. This ideal value assumes complete conversion of reactants to products without side reactions or losses. The theoretical yield depends on the limiting reactant, which is the reactant that gets completely consumed and restricts the amount of product formed. To calculate the theoretical yield, write the balanced chemical equation, convert given masses of reactants into moles, determine the limiting reactant, calculate the moles of product formed using stoichiometry, and finally convert the moles of product formed into the desired unit using its molar mass.

Step by step solution

01

Define Theoretical Yield

The theoretical yield is the maximum amount of product that can be formed from a given set of reactants in a chemical reaction based on the stoichiometric ratios of the balanced chemical equation. It is an ideal value that assumes complete conversion of the reactants to the products without any side reactions or losses.
02

Explain Limiting Reactant

In a chemical reaction, the reactant that gets completely consumed and limits the amount of product that can be formed is called the limiting reactant. It is determined by comparing the mole ratios of the reactants to the balanced chemical equation. Whichever reactant runs out first limits the formation of the product, thus affecting the theoretical yield of the reaction.
03

Relationship between Theoretical Yield and Limiting Reactant

The theoretical yield of a reaction depends on the limiting reactant because it is the reactant that determines the maximum amount of the product that can be formed. If there were an excess of the limiting reactant, more product could have been formed. Hence, the theoretical yield is based on the amount of limiting reactant present in the reaction.
04

Calculating Theoretical Yield

To calculate the theoretical yield, follow these steps: 1. Write the balanced chemical equation for the reaction. 2. Convert the given masses (or moles) of each reactant into moles using their molar masses. 3. Determine the limiting reactant by comparing the mole ratios of the reactants based on the balanced chemical equation. 4. Calculate the moles of product formed using the stoichiometry from the balanced chemical equation with respect to the limiting reactant. 5. Convert the moles of product formed into the desired unit (grams or other units) using its molar mass. The theoretical yield can be reported as moles or mass, depending on the requirement.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of \(\mathrm{FeO}\) and \(\mathrm{Fe}_{2} \mathrm{O}_{3}\). In a certain experiment, \(20.00 \mathrm{g}\) iron metal was reacted with \(11.20 \mathrm{g}\) oxygen gas. After the experiment, the iron was totally consumed, and 3.24 g oxygen gas remained. Calculate the amounts of \(\mathrm{FeO}\) and \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) formed in this experiment.

Maleic acid is an organic compound composed of \(41.39 \%\) C, \(3.47 \%\) H, and the rest oxygen. If 0.129 mole of maleic acid has a mass of \(15.0 \mathrm{g},\) what are the empirical and molecular formulas of maleic acid?

A \(9.780-\mathrm{g}\) gaseous mixture contains ethane \(\left(\mathrm{C}_{2} \mathrm{H}_{6}\right)\) and propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right) .\) Complete combustion to form carbon dioxide and water requires 1.120 mole of oxygen gas. Calculate the mass percent of ethane in the original mixture.

A 0.4230-g sample of impure sodium nitrate was heated, converting all the sodium nitrate to 0.2864 g of sodium nitrite and oxygen gas. Determine the percent of sodium nitrate in the original sample.

The compound \(\mathrm{As}_{2} \mathrm{I}_{4}\) is synthesized by reaction of arsenic metal with arsenic triiodide. If a solid cubic block of arsenic \(\left(d=5.72 \mathrm{g} / \mathrm{cm}^{3}\right)\) that is \(3.00 \mathrm{cm}\) on edge is allowed to react with \(1.01 \times 10^{24}\) molecules of arsenic triiodide, what mass of \(\mathrm{As}_{2} \mathrm{I}_{4}\) can be prepared? If the percent yield of \(\mathrm{As}_{2} \mathrm{I}_{4}\) was \(75.6 \%\) what mass of \(\mathrm{As}_{2} \mathrm{I}_{4}\) was actually isolated?
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation

Chemistry Branches

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.