Answered: If 6.58 mol of C3H1, reacts with excess…

If 6.58 mol of C3H1, reacts with excess O,, how many moles of CO, will be produced by the following combustion reaction? C;H12 + 80, → 6 H,O + 5CO, moles of CO,: 0 mol * TOOLS

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 9A

See similar textbooks

Related questions

Q: If I have a beaker with sodium carbonate which weighs 31.16g mass of the empty beaker is 29.08g what…

A: Since mass of empty beaker is 29.08 g Hence mass of sodium carbonate = mass of beaker with sodium…

Q: 1. Given the following reaction: (Balance the equation first!) _C;H; _co, _H,0 -------> a) If you…

A: We will try my best

Q: Given the balanced equation: Zn + 2 HCI ---> ZnCl, + H, How many grams of hydrogen gas (H,) will be…

A: Zn(s) + 2HCl(aq) → ZnCl2, (aq) + H2 (g) 1 mole of Zn reacts with 2 moles of HCl to produce 1 mole…

Q: 1. Zinc. Zın, reacts with Sulfur, S,according, to the reaction: Zn + Sn - Zns Balance the chemical…

Q: and abrasions. In the laboratory, small quantities of hydrogen perox can be prepared by the action…

A: Given, Chemical Reaction: BaO2 (s) + 2HCl (aq) ---> H2O2 (aq) + BaCl2 (aq) Mass of BaCl2 =…

Q: Each step in the following process has a yield of 70.0%. CH, + 4CI, - CCI, + 4 HCI CCI, + 2 HF -…

Q: 6. Li+H,O-LIOH H2 Balanced Equation: Reaction Type: Molar Masses Li H,O LIOH H In this reaction, it…

A: Please note- As per our company guidelines we are supposed to answer only one question. Kindly…

Q: 3.93 When combined, aqueous solutions of sulfuric acid andpotassium hydroxide react to form water…

A: The balanced chemical equation is: H2SO4(aq) + KOH (aq) → H2O (l) + K2SO4 (aq)

Q: In certain reaction Fe and O2 combine to form irom(III) oxide. 10.7 mole of Fe and 10.4 mole of O2…

A: Balanced chemical equation: 4Fe(s) + 3O2(g) ------> 2Fe2O3 This shows 4 moles of Fe reacts with 3…

Q: Aluminum oxidizes according to the following equation: Al + O2 -----> Al2O3 a. Powdered Al…

Q: 4. Given the reaction N,+ H, à NH, How many grams of O, will you get if 4.2g of N,reacts with excess…

A: Use stoichiometric calculation to find the mass of ammonia formed from N2 in excess of hydrogen gas.

Q: 5. CHgOH + O2- CO, H,0 Balanced Equation Reaction Type: Molar Masses CHgOH CO2 H2O In this reaction,…

A: As there are three different questions, I am solving the first one only. If you want the solution to…

Q: If 6.58 g of product are formed in a reaction and the percent yield was 69.4 %, what was the…

A: Given: The actual yield. The % yield = 69.4 %.

Q: component of advanced batteries is lithium nitride, Li3N. The reaction to form Li3N from lithium…

Q: MOLES OF A SUBSTANCE In the following reaction: 4 FeS + 7 0, --->2 Fe,O, + 4 SO, a. How many moles…

A: Answers given as do follow

Q: The corrosion of aluminum in cookwares is prevented as the aluminum metal reacts with oxygen in the…

A: Reaction is said to be balanced if there are equal number of atoms on both sides of the reaction.

Q: 9 Consider the following reaction: 4 Li + 3 0, ----> 2 LizO3 10.0 g Li and 10.0g O2 are allowed to…

A: (a) The number of grams of Li2O3 - => ( 10.0 g Li) × (2×62 g mol-1 Li2O3 )/(4×7 g mol-1 Li) =>…

Q: Determine the limiting reactant in the reaction. Calculate the amount in grams of CO2 from thew…

Q: Each step in the following process has a yield of 90.0%. CH, + 4Cl, CCI, + 4 HCI CCI, + 2 HF → →…

Q: # 9. A chemist wishes to make 5.00g of CuCl216) by the reaction: CuClzac) + Na,S03 ag) + H,O → CuCle…

A: Actual yield of CuCl = 5.00 g Percent yield = 85.0 %

Q: Limestone(CaCO3) is used to remove acidic pollutants from smokestack flue gases in a sequence of…

A: Given: Mass of coal combusted = 69000 Kg Percent by mass of sulfur in coal = 0.42 % And yield of…

Q: If 4.40 mol of C,H, reacts with excess O,, how many moles of CO, will be produced by the following…

A: C5H12 + 8O2 → 6H2O + 5CO2 From the Balanced chemical equation we get that ; 1 mol C5H12 produce = 5…

Q: The following two-step process has a 30.0 % yield for each step. CH4 + 4 Cl2 + CCL + 4 HCI CC4 + 2…

A: Given that: The % yield of each step = 30.0% Moles of CH4 used= 4.00 mol.

Q: Each step in the following process has a yield of 90.0%. CH, + 4 Cl, СС, + 4 HCI CCI, + 2 HF → ССІ,…

A: Recall the given equations CH4 + 4Cl2→ CCl4 + 4HClCCl4 + 2HF→ CCl2F2 + 2HClEach step in the…

Q: If 4.11 mol of C,H, reacts with excess O,, how many moles of CO, will be produced by the following…

Q: Suppose that exactly 5.25g of each reactant is taken. Determine which reactant is limiting, and…

A: Manganese oxide reacts with sulfuric acid to form manganese sulfate and water. The equation for the…

Q: B. The neutralizing reaction between hydrochloric acid and calcium hydroxide produces calcium…

A: Given Mass of Ca(OH)2 = 0.65 gram Molar mass of Ca(OH)2 = 40 + ( 2×17 ) gm/mole…

Q: Consider the follarina unbalanced equation: Caz POA),S)+H, SO4 @e>CaSO45)+H; PO4 @c) What masses of…

A: The given unbalanced equation is: Ca3(PO4)2 + H2SO4 -----> CaSO4(s) + H3PO4 Balancing the…

Q: Each step in the following process has a yield of 70.0%. CH, + 4 Cl, → CCl, + 4 HCl CCI, + 2 HF →…

A: The total amount of HCl produced by the given reaction has to be calculated,

Q: Suppose 1.1780g CuCl, and 2.2773g of Na,PO, were reacted as in this experiment. What is the…

Q: How many moles of NH, can be produced from 4.10 moles of nitrogen in the following reaction: N, (g)…

A: We will use mole concept to solve above problem.

Q: 9. Aluminum chloride AICIB is on ieerpunsive reagent used in many industrial processes It by…

A: According to the question, Aluminium metal reacts with chlorine gas to produce AlCl3 (Aluminium…

Q: One of the commercial uses of sulfuric acid is in the production of calcium sulfate and phosphoric…

A: For the given reaction, Ca3(PO4)2 (s) + H2SO4 (aq) → H3PO4 (aq) +CaSO4 (aq) Mass of Ca3(PO4)2 = 26.8…

Q: 2.Small amounts of oxygen gas can be produced for laboratory use by heating potassium chlorate,…

A: The amount of the reactant or products used in a reaction can be calculated from the balanced…

Q: c) Acetylene, C,H, is the fuel used for welding. i) Write the skeleton equation for the combustion…

A: 1) C2H2(g) + O2(g) =CO2(g) +H2O(g) 2)C2H2(g) + 5/2O2(g) =2uCO2(g) +H2O(g)

Q: How much LiI is produced when 350.0 g of HI reacts completely with LiOH, according to the equation…

A: Calculate the number of moles of HI. Number of moles = Given massMolar massNumber of moles of HI =…

Q: Gold(III)hydroxide is used for electroplating gold onto other metals. It can be made by the…

A: Given 20g of KAuCl4 is mixed with 25g of Na2CO3 , we have to tell what mass of Au(OH)3 will be…

Q: * 00 0.0 When glucose (C 6H1206) reacts with molecular oxygen, Gaseous carbon dioxide and liquid…

A: Given, The combustion of glucose(C6H12O6) with molecular oxygen to form gaseous carbon dioxide and…

Q: 4. 15.4 g of methanol (CH.OH) reacts completely according to the following reaction: CH.OH (g) →…

A: from Balanced chemical equation using mole concept we easily find how much moles of reactent is used…

Q: Some rocket engines use a mixture of hydrazine, N2H4, and hydrogen peroxide, H2O2, as the…

Q: Wine goes bad soon after opening because the ethanol (CH,CH,OH) in it reacts with oxygen gas (0,)…

Q: 4 IfI produce 0.5 grams of CO2, how many moles of C3HS reacted?

A: The balanced chemical equation for the combustion of C3H5 can be written as: 2C3H5 + 172O2 →…

Q: if 4 miles of barium hydroxide react, The reaction consumes __ miles of sulfuric acid. The reaction…

Q: how do i do this

A: The balanced chemical reaction is shown as,

Q: For the following reaction, 5.29 grams of carbon tetrachloride are mixed with excess methane (CH4).…

A: Given, Mass of carbon tetrachloride= 5.29g Mass of dichloromethane=5.40 g Solution is given below in…

Q: 1. (5 marks) In one process, 124 g of C,Hs are reacted with 480 g of O2. C,Hs + O2→ CO + H;0 Molar…

Q: 5. For each of the following unbalanced chemical equations, suppose that exactly 50.0 g of each…

A: 1.(a) The given chemical reaction is : NH3(g)+Na(s)→NaNH2(s)+H2(g) Balanced equation : 2 NH3(g)+2…

Q: Hydrocarbon mixtures are used as fuels. (a) How manygrams of CO₂(g) are produced by the combustion…

A: In a balanced chemical reaction, stoichiometry gives the relationship between the amount of…

Q: I just need a step-by-step explanation for this problem I forgot how to Calculate percent yield

A: The percentage yield of the substance can be described as the ratio of actual yield of the substance…

Q: 2. Calculate the number of moles and mass (in grams) of C,H, required to react with water to produce…

A: We have to calculate the moles and mass of C2H4 required.

Question

Please help. Thanks

If 6.58 mol of C3H12 reacts with excess O,, how many moles of CO, will be produced by the following
combustion reaction?
C;H12 + 80, → 6H,0 +5CO,
moles of CO,: 0
mol
* TOOLS
x10

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps

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

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.
Citric acid, C6H5CH3, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger . The equation representing this reaction is C12H22O11+H2O+3O22C6H8O7+4H2O What mass of citric acid is produced from exactly 1 metric ton (1.000103kg) of sucrose if the yield is 92.30%?
For each of the following incomplete and unbalanced equations, indicate how many moles of the second reactant would be required to react completely with 0. 145 mole of the first reactant. msp;BaCl2(aq)+H2SO4(aq) msp;AgNO3(aq)+NaCl(aq) msp;Pb(NO3)2(aq)+Na2CO3(aq) msp;C3H8(g)+O2(g)
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.
Methanol, CH3OH, is used in racing cars because it is a clean-burning fuel. It can be made by this reaction: CO(g)+2H2(g)CH3OH(l) What is the percentage yield if 5.0103gH2 reacts with excess CO to form 3.5104gCH3OH ?
Sodium borate decahydrate, Na2B4O710H2O is commonly known as borax. It is used as a deodorizer and mold inhibitor. A sample weighing 15.86 g is heated until a constant mass is obtained indicating that all the water has been evaporated off. (a) What percent, by mass of Na2B4O710H2O is water? (b) What is the mass of the anhydrous sodium borate, Na2B4O7?
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.
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
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?
Chlorine and fluorine react to form gaseous chlorine trifluoride. Initially, 1.75 mol of chlorine and 3.68 mol of fluorine are combined. (Assume 100% yield for the reaction.) (a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) What is the theoretical yield of chlorine trifluoride in moles? (d) How many moles of excess reactant remain after reaction is complete.
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.
For each of the following balanced equations, indicate how many moles of the product could be produced by complete reaction of 1.00 g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. msp;NH3(g)+HCl(g)NH4Cl(s) msp;CaO(s)+CO2(g)CaCO3(s) msp;4Na(s)+O2(g)2Na2O(s) msp;2P(s)+3Cl2(g)2PCl3(l)