
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
![Question 2.a of 8
[Tutorial: Limiting reactant stoichiometry]
This question will walk you through the steps of calculating the mass of products
produced based on your determination of the limiting reactant.
Step 1: Evaluate the question. Which of the following correctly describes a limiting
reactant?
A) The reactant with the lower mass
B) The reactant with the greater mass
C) The reactant with fewer moles
D) The reactant with greater moles
E) The reactant that runs out first, causing the
reaction to stop](https://content.bartleby.com/qna-images/question/23f54c76-b762-419b-8fbe-ee40e7662c11/5285a515-cf07-4f7f-8709-1b0d7ac09b09/ki80mw_thumbnail.jpeg)
Transcribed Image Text:Question 2.a of 8
[Tutorial: Limiting reactant stoichiometry]
This question will walk you through the steps of calculating the mass of products
produced based on your determination of the limiting reactant.
Step 1: Evaluate the question. Which of the following correctly describes a limiting
reactant?
A) The reactant with the lower mass
B) The reactant with the greater mass
C) The reactant with fewer moles
D) The reactant with greater moles
E) The reactant that runs out first, causing the
reaction to stop
Expert Solution

This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 3 steps

Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- < [Review Topics] [References) Use the References to access important values if needed for this question. For the following reaction, 0.577 moles of methane (CH4) are mixed with 0.399 moles of carbon tet methane (CH4) (g) + carbon tetrachloride (g) → dichloromethane (CH₂ Cl₂) (g) What is the formula for the limiting reactant? What is the maximum amount of dichloromethane (CH₂ Cl₂) that can be produced? Amount = mol Submit Answer Retry Entire Group 4 more group attempts remainingarrow_forwardA chemist will use a sample of 30 g of ethanol (CH3CH2OH) in an experiment. In one to two sentences, make and justify a claim about the number of moles of ethanol the chemist will usearrow_forward72.691g 84.321g FeSO4 + Potassium phosphate à Iron (II) phosphate + K2SO4 Convert the given amount of each reactant to the moles of each reactantarrow_forward
- Question 25 of 97 Submit DDT was an insecticide used to prevent mosquito borne diseases. Due to the harmful effects on birds and fish, it is now banned in the US. However, other countries still use it to control mosquitos. It can be prepared by the reaction shown below. Determine the amount of DDT that can be produced and the percent yield for this reaction. 2C6H,CI + C2HOCI, – C,4H9CI, + H20 2 3 NEXT If a company in South America started with 1175 g of chlorobenzene (C6H5CI, MW 112.55 g/mol) and 538.5 g of chloral (C2HOCI3, MW 147.39 g/mol), set up the table below that represents 100% yield with the given reaction conditions. 2C6H,CI C2HOCI, C1.H,Cls H2O Before (mol) Change (mol) After (mol) O RESET 3.132 -3.132 3.654 -3.654 7.308 0. + -7.308 10.44 -10.44 MacBook Air F12 II F8 F10 F11 000 F9 20 F3 F7 F4 F5 F6 esc F2 F1 +.arrow_forwardPure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 4.29g of magnesium co ribbon burns with 9.01g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. Incorrect What is the limiting reactant? magnesium oxygen If the percent yield for the reaction is 84.9%, how many grams of product were formed? mass of product formed tneorrect How many grams of the excess reactant remain? mass of excess reactant: garrow_forwardPure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 2.47 g2.47 g of magnesium ribbon burns with 8.71 g8.71 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? magnesium oxygen If the percent yield for the reaction is 83.4%,83.4%, how many grams of product were formed? mass of product formed: gg How many grams of the excess reactant remain? mass of excess reactant:arrow_forward
- If 24 molecules of H2 and 18 molecules of N2 are mixed and allowed to react, how many molecules of H2, N2 and NH3 would be present at the end?arrow_forwardDirections: Balance first the chemical equation below by multiplying the coeffícient to the number of atoms of each element. Then, multíply it by the atomic mass or weight. Please refer to the periodic table of elements in recording for the atomic mass or weight of the elements Involved. Besure that the total mass of the reactant is equal to the mass of the product. This is the balance equation: 2H2 02 2H20 H=4 H=4 O=2 O=2 H=4x1=D4 g/mol O=2x16=32 g/mol H=4x1=D4 g/mol O=2x16-32 g/mol 36 g/mol 36 g/molarrow_forwardAmmonia can be synthesized by the reaction: (Show your work for all the parts) (Stoichiometry) (NOTE: This question has 2 parts. Work them individually) (Sec 4.3 - Practice Exercise 4.3) 1. 3 H28 + N2B) 2 NH3B) 2(g) What is the theoretical yield of ammonia in moles when 1.8 moles of hydrogen reacts with 5.4 moles of nitrogen a) 16.6 g of hydrogen reacts with excess of nitrogen and if the actual yield is 18.2 g, What is the percent yield? b)arrow_forward
- Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.51 g of magnesium ribbon burns with 8.71 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? magnesium oxygen If the percent yield for the reaction is 82.3%, how many grams of product were formed? mass of product formed: How many grams of the excess reactant remain? mass of excess reactant: g 50 garrow_forwardAccording to the following reaction, how many moles of bromine will be formed upon the complete reaction of 25.5 grams of bromine trifluoride? bromine trifluoride (g) →→→→bromine (g) + fluorine (g) moles brominearrow_forwardConverting between quantities To convert from a given quantity of one reactant or product to the quantity of another reactant or product • First, convert the given quantity to moles. Use molar masses to convert masses to moles, and use Avogadro's number (6.02 x 10 particles per mole) to convert number of particles to moles. • Next, convert moles of the given reactant or product to moles of the desired reactant or product using the coefficients of the balanced chemical equation. For example, in the chemical equation2H2 + O2-2H20the coefficients tell us that 2 mol of H2 reacts with 1 mol of Oz to produce 2 mol of H20. • Finally, convert moles of the desired reactant or product back to the desired units. Again, use molar masses to convert from moles to masses, and use Avogadro's number to convert from moles to number of particles. Reaction of hydrogen and nitrogen to form ammonia Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation 3H2(g) +…arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY

Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning

Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning

Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning

Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY