C4H10 (g) +02(g) → CO2 (g) + H2O (1) 1) Balance this reaction equation 2) Calculate the mass of CO2 produced when 10.5 g of C4H10 react with 15.0 g of 02. What is the experimental yield if the percent yield in one experiment is found to be 75.5%?

C4H10 (g) +02(g) → CO2 (g) + H2O (1) 1) Balance this reaction equation 2) Calculate the mass of CO2 produced when 10.5 g of C4H10 react with 15.0 g of 02. What is the experimental yield if the percent yield in one experiment is found to be 75.5%?

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: Combustion of 7.73 mg of an unknown substance yields 13.3 mg CO2 and 4.06 mg H;O. The unknown…

A: Given: Compound contains only C, H and O. Mass of compound combusted = 7.73 mg = 0.00773 g…

Q: The following reaction can be used to convert carbon dioxide to oxygen gas. 4 KO2 (s) + 2 CO:(g) → 2…

A: Given : Theoretical yield of O2 = 0.313 g Percent yield of reaction = 83.4 %

Q: In an experiment, 5.25 g of H2 was added to react with 12.5 g of O2. This produced 13.5 g of H2O.…

A: Given that, Mass of H2 = 5.25 g, Molar mass = 2 g mol-1 Mass of O2 = 12.5 g, Molar mass = 32 g…

Q: As of 2018, ~95% of hydrogen is produced from fossil fuels. One of the most important reactions of…

A: Consider the given reaction is as follows; CH4 g + H2Og → COg + 3 H2 g Given…

Q: Consider the following balanced chemical equation: 2NH3(g) + 5F2(9) 4 N2F4(9) + 6HF(g) Determine the…

A: Mass of NH3 = 78.60 g Mass of F2 = 78.60 g Known values Molar Mass of NH3 = 17 g Molar Mass of F2 =…

Q: Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) →…

A: Given : Mass of sucrose = 35.4 gram Molar mass of sucrose = 342 gm/mole

Q: Consider this balanced equation: 5O2(g)+2CH3CHO(I)→ 4CO2(g)+4H2O(I) If 23.7 moles of O2(g) and…

A: Given No.of moles of O2 = 23.7 mol No.of moles of CH3CHO = 12.7 mol No.of moles of CO2…

Q: 1. Consider the balanced chemical equation: 2 C2H2(g) + 5O2(g) → 4 CO2(g) + 2 H2O(g) How many grams…

A: Given, Mass of O2 = 25.0g

Q: This question will walk you through the steps of determining which reactant is limiting based on a…

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

Q: A sample of 1.544moles of methane (CH4) is mixed with 1.273 moles of chlorine. What is the…

A: Given :- number of moles of CH4 = 1.544 mol number of moles of Cl2 = 1.273 mol To be calculated :-…

Q: Indicate which equation should be used to calculate the % yield of a reaction. Then, assuming you…

A: Theoretical yield of a reaction: It is defined as the amount of product formed from the…

Q: 4. The combustion of ethanol (C₂H5OH) produces carbon dioxide and water. In the reaction, 3.50 g of…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: If 3.0 grams of KClO3 are reacted and 1.5 gram of KCl is actually collected, what is the percent…

Q: Consider the balanced chemical reaction below. If 24.3 g of iron is produced when 50.0 g of…

A: The amount of substance is usually defined in terms of mole. The mole is the SI unit of the quantity…

Q: Consider the following balanced chemical equation: 2NH3(g) + 5F2(g) → N2F4(g) + 6HF(g)…

Q: Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the…

A: It is based on the concept of stoichiometry and limiting reagent. Here we are required to find the…

Q: Macmillan Learning Consider the reaction. 2 Pb(s) + O₂(g) An excess of oxygen reacts with 451.4 g of…

A: Given reaction is2Pb(s) + O2(g) -------> PbO(s)Mass of lead reacted = 451.4 g Mass of lead oxide…

Q: The following reaction can be used to convert carbon dioxide to oxygen gas. 4 KO₂ (s) + 2 CO₂(g) →…

A: Percent yield of any reaction is given by

Q: Consider the reaction below: PCl3(g) + Cl2(g) PCl5(g) if 76.2 g of PCl5 are formed when 56.0 g…

Q: If 13.2 g of NH3 is collected following the reaction of 2.88 mol NO with,7.00 mol H2, calculate the…

A: Given: Mass of NH3 formed experimentally = 13.2 g. Moles of NO taken = 2.88 mol. Moles of H2 taken =…

Q: The following reaction can be used to convert carbon dioxide to oxygen gas. 4 KO₂ (s) + 2 CO₂(g) → 2…

A: Given -> 4KO2(s) + 2CO2(g) -----> 2K2CO3(s) + 3O2(g) Weight of KO3 = 0.838 gm Percent yield=…

Q: consider the following balanced equation. N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) Determine the…

A: Given, N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) Given, mass of N2O4 react = 60.0 g mass of N2H4…

Q: The expected yield of a reaction was 0.407 g. If the actual yield turned out to be 0.20, what is the…

Q: For the following reaction, 4.42 grams of carbon disulfide are mixed with excess chlorine gas. The…

Q: 2Fe(s) + O2(g) →2FeO(s) If there is 10.01 g Fe and excess O2 present, the reaction yields 9.72 g…

Q: 2Al (s) + 3Cl2 (g) --> 2AlCl3 (s) (balanced) When 46 grams of aluminum react, the actual yield is…

Q: Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) →…

A: Given - Un - Balanced Chemical equation is - C₁₂H₂₂O₁₁(s) + O₂(g) → CO₂(g) + H₂O(l) The balanced…

Q: For this chemical equation: 3 Fe(s) + 2 O2lg) → Fe;O4(s) When 14.5 g Fe and 11.2 g of O2 are…

A: The balanced chemical equation under consideration is as follows: 3 Fes+ 2 O2 g→Fe3O4 s The molar…

Q: When ethane, C₂H6, reacts with chlorine, Cl₂, the main product is C₂H5CI, but other products…

A: Given ,

Q: Consider the balanced chemical reaction below. If 24.3 g of iron is produced when 50.0 g of…

A: Given: Mass of Fe=24.3 g Mass of CO=50.0 g Mass of Fe2O3=50.0 g To find: Theoretical yield of given…

Q: Consider the reaction. 2 Pb(s) + O₂(g) 2 PbO(s) An excess of oxygen reacts with 451.4 g of lead,…

A: Mass of Lead = 451.4 gMass of forming lead (II) oxide = 361.0 gand reaction, 2Pb(s) + O2…

Q: what is the percent yield of the sulfuric acid?

A: Percent yield = (actual yield/theoretical yield) x 100%

Q: Ammonia gas can be prepared by the following reaction: CaO (s) + 2 NH4Cl(s) → 2 NH³ (g) + H₂O(g) +…

A: Given, the theoretical yield of NH3 = 191 g The actual yield of NH3 = 133 g We have to calculate the…

Q: How many g of CO, will be produced by the combustion of 6 mol of ethanol?

A: Given:- C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g) Number of moles of ethanol = 6 mol To be…

Q: Combining 0.288 mol Fe,0, with excess carbon produced 16.2 g Fe. Fe,0, +3C – 2 Fe + 3 CO What is the…

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

Given the following reaction equation:
C4H10 (g) + 02(g) → CO2 (g) + H2O (1)
1) Balance this reaction equation
2) Calculate the mass of CO2 produced when 10.5 g of
C4H10 react with 15.0 g of 02.
What is the experimental yield if the percent yield in
one experiment is found to be 75.5%?

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: Introduction

VIEW

Step 2: Net Balanced reaction

VIEW

Step 3: Calculate mass of CO2

VIEW

Step 4: Calculate experimental yield

VIEW

Solution

VIEW

Step by step

Solved in 5 steps with 10 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

Consider the following balanced equation, an important reaction in the industrial manufacture of phosphorus pentachloride:PCl3(g) + Cl2(g) → PCl5(g)This reaction has a known yield of PCl5 of 66.3%. You are a chemical engineer tasked with producingPCl5. Determine the actual mass of phosphorus pentachloride formed when you react 61.3 kg ofmolecular chlorine with an excess of phosphorus trichloride. (P: 30.97 g/mol; Cl: 35.45 g/mol)
8. Consider the following reaction: 5A + 3B --> 2C + 2D 10.0 moles of A and 6.00 moles of B reacted and produced 3.00 moles of D. What is the percent yield of product D in this reaction?
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 +.
For the following reaction: C3H8(g) + 02 ——-> CO2(g) +H20(g) a). balance the reaction b). determine the limiting reactant from 20.0 grams of each starting reactant c). calculate the theoretical yield of CO2(g) in grams d). calculate the percent yield if the actual yield was 10.7 grams
2. Ethyl chloride is prepared by the reaction of chlorine with ethane according to the following equation: C:Ho(g) + Cl2(g) – CH$CI(g) + HCl(g) Ethane Ethyl chloride a) Write the balanced chemical equation. Show proof of completion. b) When 5.6 g of ethane is reacted with excess chlorine, determine its theoretical yield c) Calculate the percent yield of ethyl chloride if experimental results indicated that 8.54 g of ethyl chloride had formed.
Sodium and chlorine react to form sodium chloride: What is the theoretical yield of sodium chloride for the reaction of 32.0 g Na with 107.2 g Cl2? 1.40 x 104 g NaCl 35.4 g NaCl 122 g NaCl 81.2 g NaCl
Dichlorine monoxide, Cl,0, is sometimes used as a powerful chlorinating agent in research. It can be produced by passing chlorine gas over heated mercury(I) oxide according to this equation: HgO+Cl2 → HgCl, + Cl20 What is the percent yield, if the quantity of reactants is sufficient to produce 8.90 g of Cl,0 but only 2.10 g is obtained? Answer in standard notation to the nearest tenth of a percent
fill in blanks and solve using the emthod shown! please
Part one What is the percent yield if 15.0 grams of iron was obtained from Fe production when65.0 grams of iron (III) oxide is reacted with 52.3 grams of carbon monoxide accordingto the following balanced reaction? Equation: Fe2Og(s) + 3 CO(g) -> 2 Fe(s) + 3COn(g). part two