Determine the total mass of the product that could be formed from the balanced reaction shownbelow by constructing a BCA table and determining the maximum grams of product that can beproduced. Complete Parts 1-2 before submitting your answer.2 Al +31,-2 All,NEXTAssume the reaction starts with 4.20 g Al (26.98 g/mol) and 17.40 g iodine, I, (MW 253.80 g/mol). Set up the table belowthat represents 100% yield with the given reaction conditions..2 Al+31,2 AllBefore (mol)Change (mol)After (mol)0-0.1030.1030.1560.110-0.15-0.1100.0060.0534.0680-0.05300457RESET--00457Submit

Answered: Image /qna-images/answer/eeb6af16-f944-47b9-8126-a8a4046a8739.jpg

2 Al +31,-2 All, 2 NEXT Assume the reaction starts with 4.20 g Al (26.98 g/mol) and 17.40 g iodine, I, (MW 253.80 g/mol). Set up the table below that represents 100% yield with the given reaction conditions.. 2 Al 31, 2 All, Before (mol) Change (mol) After (mol)

2 Al +31,-2 All, 2 NEXT Assume the reaction starts with 4.20 g Al (26.98 g/mol) and 17.40 g iodine, I, (MW 253.80 g/mol). Set up the table below that represents 100% yield with the given reaction conditions.. 2 Al 31, 2 All, Before (mol) Change (mol) After (mol)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: What amount (in mol) and what mass (in g) of water can be produced when 82.1 ug of ethane reacts…

A: The reaction considered is, C2H6 (g) + O2(g)→H2O(l)+CO2(g) The balanced equation of this reaction…

Q: Find the limiting reactant for each initial amount of reactants. Drag the appropriate items to their…

Q: Page < 4. Using the following reaction, how many moles of CO will be produced when 4.7 moles of C…

Q: . Na H2O S NaOH H2 24. KClO3 S KCl O2 25. Fe3O4 C S Fe CO 26. C5H8 O2 S CO2 H2O 27. Cu…

A: Balanced chemical equation is the equation in which number of atoms on both sides of equation are…

Q: 25. Zinc oxide reacts with water to form zinc hydroxide. If 0.25 mol of zinc oxide is reacted with…

A: Moles of Zinc oxide(ZnO) = 0.25 molMoles of water = 0.25 molMoles of Zinc hydroxide (Zn(OH)2)…

Q: If you are running the reaction below and you have excess K and 0.16 mol Cl2, what mass of KCl will…

Q: 2a+4b----> 3c

A: C. 96 (96 moles of C form o complete reaction of 64 moles of A.)

Q: Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs,…

Q: ChatGPT ChatGPT To determine the amount of Al2O3Al2O3 produced from the reaction of 0.30…

A: The objective of the question is to determine the amount of Al2O3 produced from the reaction of 0.30…

Q: 2 KCIO316) ------> 2 KCI5) + 302(g) How many moles of KCI are produced when 1 mole of KCIO3…

A: The given reaction is , 2 KClO3 (s) ------> 2 KCl (s) + 3…

Q: An experiment was carried out to make potassium dichromate(VI) from chromium(III) potassium sulfate…

A: To determine the moles of chromium(III) potassium sulfate (chrome alum) used in the experiment, you…

Q: Now, set up a limiting reactant problem to determine how many grams of your precipitate (AgCl) you…

A: 1. Recall the given reaction, AgNO3 aq + NaCl aq → AgCl s…

Q: Averages using the table* average of NaOH used In liters average moles of NaOH used (mol)…

A: The volume of NaOH used in trial 1, trial 2, and trial 3 is 47.98 mL, 47.12 mL, and 47.12 mL,…

Q: Consider thecombustion reaction. C3H8 + 5O2--------3CO2 + 4H2O Ifyou react 15.0 mol of O2 how many…

A: The balanced combustion reaction is given by

Q: These images show equal moles of So2 gas and o2 gas about to be mixed to form So3. 8. Assuming the…

A: Given : Some statements regarding the reaction between sulphur dioxide and oxygen to form sulfur…

Q: For the balanced equation below, someone combines 49.7 g of ammonium sulfate (molar mass = 132.16…

A: Given, (NH4)2SO4 + Ca(OH)2 → 2NH3 + CaSO4 + 2H2O mass of Ammonium sulphate, (NH4)2SO4 react = 49.7 g…

Q: Consider this reaction: Mg + 2HCI --> H2 + MgCl2 How many moles of H2 will form from 26 moles of…

A: From the reaction it is clear that one mole of Mg reacts with two moles of HCl to form two moles of…

Q: Question 18 Note: This is a follow-up question on question 17 above. Consider the following balanced…

A: This question can be solved by identifying the limiting reagent and excess reagent by calculating…

Q: If this reaction is conducted with 57.4 g CoCl₂ and 42.0 g F₂, how many grams of I mol Cla= 129.8…

Q: True of False, actual yield and theoretical yield will usually be the same. O True because…

A: Answer:Theoretical yield is the maximum amount of product that can be obtained from the given amount…

Q: sider the generic chemical equation: 2 A + 3 B moles of A and 2 moles ofB are reacted, what is the…

Q: When this chemical equation is balanced, the coefficient in front of H₂O is? Na + H₂O -----> NaOH +…

Q: Consider the following balanced reaction: Pb(s) + 2 Cl;(g) → P6CI,(s) Starting with 30.0g of Cl2 and…

A: Consider the following balanced reaction: Pb(s) + 2Cl2(g) → PbCl4(s) The mass of Cl2 given = 30.0 g…

Q: For the following reaction, 0.139 moles of sulfur are mixed with 0.467 moles of carbon monoxide.…

A: It is based on the stoichiometry. Here we are required to find the maximum amount of sulphur…

Q: The molar mass of glucose is 180.2 g/mol. How many grams of glucose will be produced when 132.0g of…

Q: 42. How many grams of H,0 will be formed when 42.0 g H, is mixed with 38.0 g 02 and allowed to react…

A: Since you asked specific question so as per Q&A guidelines of portal I solved Question number 42…

Q: Determine the number of molecules of Cr₂O3 that form when 1.34 x 10³ g of oxygen completely reacts…

Q: 1. Consider the generic reaction: A + 2B→ C How many moles of C are formed upon the complete…

A: Hello. Since your question has multiple questions, we will solve the first question for you. If you…

Q: 8. A chemistry student weighed a piece of chalk and found that it had a mass of 56.7 g. After a day…

A: Given in the question, Mass of chalk before using = 56.7 gm Mass of chalk after using = 48.3 gm Mass…

Q: None

Q: mass fraction:

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

Determine the total mass of the product that could be formed from the balanced reaction shown
below by constructing a BCA table and determining the maximum grams of product that can be
produced. Complete Parts 1-2 before submitting your answer.
2 Al +31,-2 All,
NEXT
Assume the reaction starts with 4.20 g Al (26.98 g/mol) and 17.40 g iodine, I, (MW 253.80 g/mol). Set up the table below
that represents 100% yield with the given reaction conditions..
2 Al
+
31,
2 All
Before (mol)
Change (mol)
After (mol)
0
-0.103
0.103
0.156
0.110
-0.15
-0.110
0.006
0.053
4.0680
-0.053
00457
RESET
--00457
Submit

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!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

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

What is the conversion factor between two different substances in a chemical reaction? 81°F Mostly sunny Esc F1 1 {0 atomic numbers mole ratio molar mass F2 mass ratio -8- @ 2 F3 -Ő+ #M 3 FA 54 $ F5 % 5 F6 T Q F7 < 6 F8 & 7 F9 ★ * 00 8 F10 9 F11 ) F12 a P Prt Sc
Percent yield. 4Fe + 3O2 ---> 2Fe2 O3 Starting with 320g of oxygen gas you produce 75g of Iron(iii) oxide. What is the percent yield?
In initial state before CH4 and Cl2 is shown in the figure based on the balance equation in the future what is the limiting reactant? A. CCL4 B. CH4 C. HCL D. CL2
calculate how many moles of products would be produced if 0.500 mole of the first reactant were to react completely.
Consider the following Reaction 4 KOH +6KMnO4+10CrCl3+7H2O-->6MnCl2 +5K2Cr2O7+18HCl how many moles of MnCl2 are formed starting with one mole of each reactant?
Right in the same form as a question please (balancing and stoichiometry)
a reaction mixture initially contains 0.25 moles of ZnS and 0.25 moles of O2. after the reaction is complete. how many ,oles of the excess reactant are left over? 2 ZnS+3 O2---> + 2 SO2 0.250 moles O2 0.125 moles O2 0.083 moles ZnS 0.167 moles ZnS
Given that 4 NH3 + 5 O2 → 4 NO + 6 H2O,when 4.50 mol of H2O are formed, the amountof NO formed isA) 3.00 mol B) 6.75 molC) 1.50 mol D) 4.50 mol
43. Find the limiting reactant for each initial amount of reactants. MISSED THIS? Read Section 4.40; Watch KCV 4.4, IWE 4.6 2 Na(s) + Br2(g) → 2 NaBr(s) a. 3 mol Na, 1 mol Br₂ b. 2.8 mol Na, 1.1 mol Br₂ c. 1.5 mol Na, 2.1 mol Br₂ d. 11.5 mol Na, 5.5 mol Br₂
3Ba(NO3)2 + 2Na3PO4 -> Ba(PO4) + 6Na(NO3)2 1) Determine the Mass of precipitate produced when excess barium nitrate is reacted with 30.5g of sodium phosphate 2) Determine the number of barium nitrate molecules that would be needed to react ----------------------------------------------------------------------------------- C3H8 + 5O2 ----> 3CO2 + 4H20 1) Determine the Mass of oxygen that would be needed to combust 4.55 x 10^23 molecules of propane (C3H8) 2) Calculate the mass carbon dioxide produced
4Fe +30₂ ----> 2Fe₂O3 YOUR TASK: • Setup and solve the following two mole-mole stoichiometry problems. 1. If you need to make 1.56 moles of Fe₂O3, how many moles of iron (Fe) will you need? 2. If you need to make 1.56 moles of Fe₂O3, how many moles of oxygen (0) will you need? Solving Mole Conversions Using Dimensional Analysis 03 9 05 WRITE DOWN THE MUMBLED UNITS GIVEN MULTIPLY BY FRACTION AR IDENTIFY THE DESIRED UNITS MATCH UNITS ON THE TOP BOTTON OF THE FRACTION BAR INSERT NUMBERS THAT BELONG WITH EACH UNIT IN THE FRACTION MULTIPLY THE NUMERATORS MULTIPLY THE DENOMINATORS SIMPLIFY THE FINAL FRACTION