Be sure to answer all parts. Given the reaction represented by the balanced equation CH(g) + 3Bry(g) –→ 3HB1(g) + CHBry(g) Part 1 out of 2 Calculate the number of g of CHBR3 produced by mixing 131 g Br; with excess CH4. CHBRY 1 attempt left Check my work Next part

Be sure to answer all parts. Given the reaction represented by the balanced equation CH(g) + 3Bry(g) –→ 3HB1(g) + CHBry(g) Part 1 out of 2 Calculate the number of g of CHBR3 produced by mixing 131 g Br; with excess CH4. CHBRY 1 attempt left Check my work Next part

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 75AP

See similar textbooks

Related questions

Q: Stoichiometry Test 16. Determine the limiting and excess reactant in the equation below if you start…

Q: The ratio of Molar masses of CH1206 and Water is 0.1:10 O 342:18 O 10:1 O 180:10 When Chloride(CI)…

A: A precipitation reaction is the reaction with the formation of an insoluble salt when two soluble…

Q: If 108 g of PCI5 are formed from the reaction of 60.3 g Cl2 with excess PCI3, what is the percent…

A: Given, Mass of Cl2 = 60.3g Mass of PCl5 = 108g

Q: C What mass of O2, in grams, is required for complete combustion of 39.0 g of methane? Mass = 155.52…

A: First of all we will calculate the moles of CH4

Q: 3. CH + 202 co, + 2H,0 2 grams Using the balanced equation above, what amount of oxygen is needed to…

A: The given balanced reaction is, CH4 + 2O2 ---> CO2 + 2H2O

Q: po Combining 0.212 mol Fe₂O3 with excess carbon produced 15.1 g Fe. Fe₂O3 + 3C 2 Fe + 3 CO What is…

Q: How many moles of C are formed upon complete reaction of 2 mol of B according to the generic…

Q: If 8.00 moles of NH3 of and 10.00 moles of O2 react in the following reaction, how many moles of…

A: In the reaction one reactant is a limiting reagent, the substance that is totally consumed when the…

Q: How many grams of O2 are needed to react with 29 g of Pļaccording to the reaction below? P4 + 5 O2 →…

A: Mass of P4 = 29 g We need to determine mass of O2 needed.

Q: Be sure to answer all parts. Given the reaction represented by the balanced equation CH4(g) +…

A: Given the reaction represented by the balanced equation CH4(g) + 3Cl₂(g) → 3HCl(g) + CHCl3(g) Molar…

Q: Chromium reacts with phosporic acid according to the following balancecd equation: 2 Cr+ 2 H3PO4 ==>…

Q: How many moles of Al are necessary to form 28.6 g of AIBR3 from this reaction: 2 Al(s) + 3 Br2(1) →…

Q: 2. (2-step problem) How many grams of MNSO4 are produced from 12.3 moles of KNO2? Again, write out…

Q: 12) What mass of Fe₂O3 would react with 20.00 g of Zn? The chemical equation for this reacti 3 Zn +…

Q: C. Stoichiometry Calculations (Remember to balance equations!!) 1. How many grams of HCl are…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: esc STARTING AMOUNT ! AMB 0¹ F1 . X 3662 @ F2 1 # 80 F3 15 How many moles of aluminum are required…

Q: PCI, + 4 H,0 8. If you use 336 moles of water in an experiment, how many moles of hydrochloric acid…

A: We only answer one question from the multiple questions. Please resubmit the other questions up to 3…

Q: STOICHIOMETRY Mole-Mole Problems How many moles of HCT are needed to react with 0.87 moles of A

Q: What volume of carbon dioxide (CO2) will be produced if 2.90 moles of iron (Fe) is produced?

A: 3. Given :- Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) no.of moles of Fe produced = 2.90 mol To…

Q: 6) Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react…

Q: Dr. Fouad Al-Qaim Problem 4 (homework) What is the limiting reactant when 10.0 g of Na (fw= 23) and…

Q: A student obtained 11.1 g of Al2S3 from the following reaction. The student added 19.5 g of Sodium…

A: Given: Weight of Al2S3 = 11.1 g Weight of Na2S = 19.5 g Weight of AlPO4 = 19.5 g The given reaction…

Q: CHAPTER 4 - STOICHIOMET O Previous Page 3 of 5 Nex A sample of limestone and other soil materials…

A: Since your question has multiple parts, we will answer first question for you. If you want remaining…

Q: Question 5 Based on the following chemical equation: 2C,H2 + 502 -> 4CO, + 2H,0 How many grams of…

Q: Excess Reactant Practice You MUST show ALL work! No work = no credit! Balanced chemical equation:…

A: The balanced chemical reaction is: CuSO4 + Zn → Cu + ZnSO4 mole of CuSO4 = 5.00 mol mole of Zn…

Q: According to the balanced reaction below, calculate the quantity of moles of NO2 gas that forms when…

Q: _CioHe + _Oz → _CO, + _H,0 late the mass of KCN formed when 27.35 g of K reacts. _Mn(CN), +_K→_KCN +…

Q: How many grams of potassium nitrate, KNO3, is produced when 150g of potassium chromate, K2CrO4,…

Q: Consider the balanced chemical reaction below. What is the maximum number of grams of Ag that can be…

A: The given balanced equation is- Given data is- Initial moles of Zn = 0.570 mol Initial moles of…

Q: In the given reaction below determine the following: BaSO4 + Al(OH)3 Al2(SO4)3 + Ba(OH)2 If 25 grams…

A: Since you have posted a question with multiple sub-parts, we will solve first three subpartsfor you.…

Q: How many grams of sodium sulfate are produced when 15 moles of copper sulfate are used? 2NaOH +…

A: Given chemical equation is : 2NaOH + CuSO4 → Cu(OH)2 + Na2SO4Sodium…

Q: 1. H2SO4 + NaOH → NazSO4 + H2O a). Balance this equation (show all work

A: The given reaction is, H2SO4 + NaOH ---> Na2SO4 + H2O To balance the given reaction, we have to…

Q: If 50.0 g of H₂ and 155.0 g of O₂ react, how many moles of H₂O can be produced in the reaction…

A: The mass of H2 is 50.0 g.The mass of O2 is 155.0 g.The balanced equation is To find the moles of H2O…

Q: In the reaction below, 7.0 mol of NO and 5.0 mol of O2 are reacted together. The reaction generates…

A: Given :- number of moles of NO = 7.0 mol number of moles of O2 = 5.0 mol To…

Q: Please solve this

Q: Question 2 of 15 Calculate the theoretical yield in grams All. from the complete reaction of 113…

A: We have to calculate the theoretical yield of product.

Q: TUTOR Limiting Reactants: Full Analysis For this reaction, 4.20 g carbon (graphite) reacts with 14.4…

Q: What is the percent yield if 28.16 g of CO2 is collected from a reaction with a theoretical yield of…

A: Percent yield =To be determined Experimental Yield = 28.16 gTheoretical Yield = 112.7 g

Q: Question 17 (1.5 points) Which of the following chemical equations is balanced? O a) E3H8 + O2 → CO2…

A: The balanced chemical equation from above options is

Q: Current Attempt in Progress Given the chemical equation, 2Mg +O2→ 2MgO, when 2.2 g Mg react with…

A: The Yield Can be obtained using Concept of Limiting Reagent . The yield Is 73.6% . THE explanation…

Q: n our bodies, sugar is broken down with oxygen to produce water and carbon dioxide. For the…

A: Solution - C6H12O6 + 6O2 → 6CO2+6H2O 0.597 moles…

Q: Correct The balanced equation is: CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O(g) c What mass of O2, in grams,…

A: Number of moles is calculated by dividing the given mass with molecular mass.

Q: How many grams of silver chromate, Ag2CrO4, is produced when 150g of silver nitrate, AgNO3, reacts…

A: The balanced chemical reaction of silver nitrate and potassium chromate is as follows: 2AgNO3 +…

Q: How many molecules of carbon monoxide (CO) are needed to react with-excess trOFE) oxide (Es) to…

Q: How many moles of each reactant were used in the reaction? (can you explain how to do it) Equation:…

A: Mole is the amount of the substance that contains the same number of particles or atoms or…

Q: According to the balanced reaction below, calculate the moles of NH; gas that form when 4.2 mol of…

A: The stoichiometric coefficients of reactants and products in a balanced chemical equation represent…

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

100%

Be sure to answer all parts.
Given the reaction represented by the balanced equation
CH(g) + 3Bry(g) –→ 3HB1(g) + CHBry(g)
Part 1 out of 2
Calculate the number of g of CHBR3 produced by mixing 131 g Br; with excess CH4.
CHBRY
1 attempt left
Check my work
Next part

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 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

For each of the following unbalanced reactions, suppose exactly 5.00 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will remain after the limiting reactant is consumed. Na2B4O7(s) + H2SO4(o H3BOj(j) + Na2SO4(u CaC,(s) + H2O(/) Ca(OH)2(s) + C2H2(g) NaCl(s) + H2SO4(/> HCl(g) + Na2SO4(s) SiO2(s) + C(x) —> Si(/) + CO(g)
The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
Small quantities of oxygen gas can be generated in the laboratory by the decomposition of hydrogen peroxide. The unbalanced equation for the reaction is H2O2(uz/)-? H2O(/) + O2(g) Calculate the mass of oxygen produced when 10.00 g of hydrogen peroxide decomposes.
Consider the following generic reaction: Y2+2XY2XY2 In a limiting reactant problem, a certain quantity of each reactant is given and you are usually asked to calculate the mass of product formed. If 10.0 g of Y2 is reacted with 10.0 g of XY, outline two methods you could use to determine which reactant is limiting (runs out first) and thus determines the mass of product formed.
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
4-89 If 7.0 kg of is added to 11.0 kg of to form which reactant is in excess?
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.
onsider the balanced chemical equation :math>4Al(s)+3O2(g)2Al2O3(s). at mole ratio would you use to calculate how many moles of oxygen gas would be needed to react completely with a given number of moles of aluminum metal? What mole ratio would you use to calculate the number of moles of product that would be expected if a given number of moles of aluminum metal reacts completely?
Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation? lf 2.50 moles of A2 are reacted with excess AB, what amount (moles) of product will form? If the mass of AB is 30.0 u and the mass of A2 are 40.0 u, what is the mass of the product? If 15.0 g of AB is reacted, what mass of A2 is required to react with all of the AB, and what mass of product is formed?
What is meant by a limiting reactant in a particular reaction? In what way is the reaction “limited”? What does it mean to say that one or more of the reactants are present in excess? What happens to a reaction when the limiting reactant is used up?
One mol of ammonia reacts with 1.00 mol of oxygen to form nitrogen oxide and water according to the reaction 4NH3(g)+5O2(g)4NO(g)+6H2O(l)State which statements are true about the reaction and make the false statements true. (a) All the oxygen is consumed. (b) 4.00 mol NO are produced. (c) 1.50 mol H2O are produced. (d) The description of the experiment does not provide enough information to determine percent yield. (e) Three moles of water are produced for every two moles of NO obtained.