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
Related questions
Concept explainers
Question
thumb_up100%
In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation:
Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g)
The molar masses for each compounds in the equation are as follows;
PCl5: 208.224 g/mol
H2O: 18.015 g/mol
H3PO4: 97.994 g/mol
HCl; 36.45 g/mol
What is the limiting reagent in this scenario?
Note! Make an accurate claim: The limiting reagent in this scenario is _____. Provide additional details and use subject specific language.
Cite evidence from what's given to you in the problem that supports your answer, hint: look at that equation!. Lastly! Fully connect the evidence to the claim/your answer to the question. Include subject specific language in your reasoning.
Your written response should LOOK exactly like the response attached. The other image is there to show how you would figure out the limiting reagent.
Transcribed Image Text:Scenario #1
How many grams of silver chloride (AgCl) are produced from the reaction between
100.0 g of silver nitrate (AgNO,) and 100.0 g barium chloride (BaCl₂) ??
2AgNO3(s) + BaCl₂ (s)
moles
liters
100.0 g
100 g BaCl2 x
100.0 g
Determine the number of moles of product that can be created from 100 g of AgNO₂:
100.0 g-AgNO3 x
1 mole AgNO3
169.87 moles AgNO3
What is the
limiting reactant?
AgNO3
Ba(NO3)2 (5) + 2AgCl (s)
0.5887 moles
1 moles BaCl2
Determine the number of moles of product that can be created from 100 g of BaCl,:
2 moles AgC!
X
1mol Bach
208.23 g BaCl2
X
2 moles AgCl
2 moles AgNO3
0.5887 moles AgCl X 143.2 g AgCl
1 mole AgCl
MOLAR MASSES IF NEEDED:
169.87 g/mol
143,32 g/mol
213.341 g/mol
208.23 g/mol
0.58868 moles
- 200/333.74= 0.5887 moles AgCl
What is the maximum amount of
AgCl that can be formed?
AgNO.
AgCl
Ba(NO₂)₂
200.0/208.23 =
84.37 g AgCl
0.960476 moles AgCl
0.9606 molos
AgCl
0.5887 moles AgCl
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 5 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
- The fizz produced when an Alka-Seltzer tablet is dissolvedin water is due to the reaction between sodium bicarbonate(NaHCO3) and citric acid (H3C6H5O72)3 NaHCO3(aq) + H3C6H5O7(aq)-------->3 CO2(g) + 3H2O(l) + Na3C6H5O7(aq) In a certain experiment 1.00 g of sodium bicarbonate and1.00 g of citric acid are allowed to react. The actual yield of CO2 was 0.436 g. a.) What is the theoretical yield of CO2? b.) What is the % yield?arrow_forwardIf 50.0 g of water is combined with 155.3 g of PCl3, PCl3(l) + 3H2O (l) --> H3PO4 (aq) + 3HCl (aq) what is the limiting reagent?arrow_forwardBalance the following reaction. If a reactant or product is not present, put a zero (0) in the blank. H+(aq) + H2O(l) + ClO-13(aq) + e-1 <--> Cl-1(g) + H+(aq) + H2O(l)arrow_forward
- 2+ Natural waters often contain relatively high levels of calcium ion, Ca²+, and hydrogen carbonate ion (bicarbonate), HCO3¯, from the leaching of minerals into the water. When such water is used commercially or in the home, heating of the water leads to the formation of solid calcium carbonate, CaCO3, which forms a deposit ("scale") on the interior of boilers, pipes, and other plumbing fixtures. Ca(HCO3)2 (aq) → CaCO3 (s) + CO2(g) + H₂O(1) If a sample of well water contains 0.0016 mg of Ca(HCO3)2 per milliliter, what mass of CaCO3 scale would 1.0 mL of this water be capable of depositing? Mass= garrow_forwardArsine, AsH3, was once a product of a test used in forensic analysis. Tissues from a possible poisoning victim were treated with zinc and sulfuric acid. If arsenic was present (usually as diarsenic trioxide, As203), arsine would form: As₂03 (s) + 6 Zn(s) + 6 H₂SO4(aq) ----> 2 AsH3(g) + 6 ZnSO4(aq) + 3 H₂O(1) a) In a lab exercise, a forensic technician reacts 19.8 g of AS₂O3 with 32.7 g of Zinc in the presence of excess sulfuric acid. What mass of AsH3 will be produced? b) Use the same chemical reaction, create a question which needs to be solved by percentage yield.arrow_forward???arrow_forward
- 16) According to the balanced chemical equation 5 H2C20 4(aq) + 2 MnO4-(aq) + 6 H+(aq) →10 CO 2(g) + 2 Mn2+(aq) + 8 H2O() 0.3500 grams of oxalic acid, H2C2O4 will react with_ _moles of permanganate, MnO4". A) 0.009718 B) 0.001554 C) 0.003887 D) 0.007774arrow_forwardDteremine the limiting reaganet (SHOW THE calculations for determinig the limiting reagent ) and calculate the theoretical mass of PbI2 by using limiting reagent. show your calculations. Balanced Equation: Pb(NO3)2 (aq) + 2KCL(aq) ---> 2KNO3(aq) + PbI2(s) No of moles of Pb(NO3)2 = 0.003 No of moles of KI = 0.007arrow_forwardThe reaction for producing glucose in plants, called photosynthesis, is 6CO2+6H2O−→−−lightC6H12O6+6O2 6CO2+6H2O→lightC6H12O6+6O2 If a plant produces 7.56 mol C6H12O6,7.56 mol C6H12O6, how many moles of CO2CO2 are needed?arrow_forward
- Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?arrow_forward4.106. Aspirin (acetlsalicyclic acid) may be formed from salicyclic acid and acetic acid as follows:C7H6O3 (aq) + CH3COOH (aq) → C9H8O4(s) + H2O(l)Salicyclic acid Acetic Acid Aspirin b. How many mol of aspirin may be produced from 1.00*102 mol mol salicylic acid? c. How many g of aspirin may be produced from 1.00*102 mol salicylic acid? d. How many g of acetic acid would be required to completely with the 1.00*102 mol salicylic acid? e. For the conditions in part (d), how many g of aspirin would form?arrow_forwardIn a particular experiment 0.0039 moles of AgNO3 is added to 0.001875 NH4Cl and 0.156g of AgCl are recovered. What is the percent yield? AgNO3(aq) + NH4Cl(aq) --> AgCl(s) + NH4NO3(aq)arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles 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 Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary 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