Given the balanced chemical reaction: 2CH3OH + 302 - 2 + 4H₂0 Use the mass of the following elements Ic H o 12.00 1.00 16.00 What is the percent yield for a process in which 10.4 g CH3OH reacts with 10.1g 02 and the actual yield is 10.0g CO2. Percent

Given the balanced chemical reaction: 2CH3OH + 302 - 2 + 4H₂0 Use the mass of the following elements Ic H o 12.00 1.00 16.00 What is the percent yield for a process in which 10.4 g CH3OH reacts with 10.1g 02 and the actual yield is 10.0g CO2. Percent

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.35PAE

See similar textbooks

Related questions

Q: Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with…

A: Given equation is 2C8H18 + 25O2→16CO2 + 18H2O Given that, Moles of C8H18 =4.000 moles Moles of…

Q: When 6.8 g al Aluminum reacts with excess oxygen according to the following balanced equation and…

A: Aluminium reacts with oxygen to form aluminium oxide as per the reaction, => Al (s) + O2 (g)…

Q: (2)For the following balanced reaction use the mass of the chemical provided to solve the mass of…

Q: Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with…

A: Number of moles of C8H18 = 4.000 moles Number of moles of O2 = 4.000 moles Balanced chemical…

Q: f the reaction of 30 grams of calcium carbonate (CaCO3) produces 15 grams of calcium oxide (CaO),…

A: CaCO3 decompose to give CaO and CO2. Reaction is as follows: CaCO3 ---------> CaO + CO2 Mass of…

Q: 2Ca + O2 -> 2CaO 3.80 g Ca and 2.90 g O2 is allowed to react and 5.20 g of CaO is formed. q1:…

A: Given: Mass of calcium = 3.80 g Mass of O2 = 2.90 g Actual yield of CaO = 5.20 g Known: Molar mass…

Q: Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The unbalanced…

A: Given: Mg(s)+O2→MgO(s) Mass of Mg=10.1 gMass of O2=10.5 gMass of MgO=11.9 g To determine: Limiting…

Q: Find the mass of O2 required to also burn.

Q: Which of the following statements is false? * The percent yield = x 100% The limiting reactant is…

A: In a chemical reaction, the limiting reactant is the reactant that gets consumed first and the other…

Q: Consider the following balanced reaction: 2C4H10 + 1302 → If 0.237 mol C4H10 and 1.65 mol O2 are…

A: given :- 2C4H10 + 13O2 → 8CO2 + 10H2O no.of moles of C4H10 = 0.237 mol no.of moles of O2 = 1.65 mol…

Q: Consider the following balanced reaction: 2C4H10 + 1302 → 8CO2 + 10H20 If 0.237 mol C4H10 and 1.65…

Q: For the reaction represented by the equation Mg + 2HCl ->H2 + MgCl2 the percentage yield of…

Q: Consider this reaction, which occurs in the atmosphere and contributes to photochemical smog:…

Q: Combining 0.329 mol Fe2O3 with excess carbon produced 18.9 g Fe Fe2O3+3C⟶2Fe+3CO What is the actual…

A: Given:0.329 mol Fe2O318.9 g FeThe chemical equation involved:Fe2O3+3C⟶2Fe+3CO

Q: Consider the reaction: 4A + 3B - 3C + 4D A student in our chemistry laboratory mixes 6.4 mol…

A: The limiting reagent in a reaction is a reactant that is totally consumed when the reaction is…

Q: According to the following reaction, how many grams of calcium carbonateare necessary to form 0.559…

A: In this question, we will determine the mass of calcium carbonate in grams unit. Given : moles of…

Q: n the reaction of 10.00 mL of FeCl3{aq) and 12.4 g of <½C2O4laq). you calculate that 9.58 g of…

A: Volume of FeCl3 = 10.00 mL Mass of K2C2O4 : 12.4 g Mass of K3FeC2O43H2O = 9.58 g

Q: If the percent yield for a given reaction is 73.23% and the theoretical yield for the same reaction…

Q: Consider this reaction, which occurs in the atmosphere and contributes to photochemical smog: 4Fe(s)…

Q: CALCIUM CARBONATE IS DECOMPOSED BY HEATING. THE BALANCED EQUATION FOR THIS REACTION IS CaCO3 ---›…

A: We know that, Percent yield = Actual yieldTheoretical yield×100% Actual yield is the amount of…

Q: In the reaction below, 7.0 mol of NO 5.0 mol O2 are reacted together. The reaction generated 3.0 mol…

A: The formula for percent yield calculation is - Percent yield = (actual yield of product/theoratical…

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: Write a balanced chemical equation based on the following description: butane gas reacts with oxygen…

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

A: In the reaction 2 moles of lead react with 1 moles of oxide to give 2 moles of lead oxide.

Q: Consider the following balanced reaction: 2C4H10+ 1302 → 8CO2+ 10H2O 0.237 mol C4H10 and 1.65 mol O2…

A: Given : We have to calculate the moles of carbon dioxide.

Q: For the reaction: Na2CO3 + CuCl2 --> CuCO3 + 2 NaCl If 25.7 grams of NaCO3 are required to form…

A: The balanced reaction is: Molar mass of Na2CO3 = 105.98 g/mol Molar mass of NaCl = 58.44 g/mol…

Q: Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced…

A: Given Reaction 2Mg(s) + O2(g) → 2MgO(s) Mass of Mg = 10.2 gram Mass of O2 = 10.6 gram Actual…

Q: For the following reaction: C3Hg(g) + O2(g) ————> CO2(g) + H2O(g) a). balance the reaction b).…

A: It is based on basic concept of physical chemistry (mole concept). Forulma used: 1mole=6.022*1023=…

Q: Combining 0.277 mol Fe2O30 with excess carbon produced 10.0 g. Fe2O3+3C⟶2Fe+3CO What…

A: Given, moles of Fe2O3 reacted = 0.277 mol and, mass of iron produced, actual yield = 10.0 g…

Q: Determine percent yield for the reaction. Magnesium oxide can be made by heating magnesium…

Q: A container holds 75.0 g of CuO and 5.00 g of H₂. The following reaction occurs: CuO + H₂ --> Cu +…

A: Theoretical yield is defined as the maximum amount of product that can be formed from the given…

Q: If 14.0 g of C₂H4 react completely to form 7.84 g of water, as shown below, the percent yield in the…

A: We can solve this problem by using this equation %yield = (observed yield / theoretical yield)× 100

Q: When 65.0 g of benzene (C,H6) burns in oxygen to give 32.9 g carbon dioxide and water are formed, if…

A: Given :- Mass of C6H6 = 65.0 g Mass of CO2 = 32.9 g Theoritical yield = 35.5 g To be calculated…

Q: You are given the balanced equation: C3HB + 5 02 - 3 CO2 + 4 H2O If 0.3618 moles of C3Hg are allowed…

A: Limiting reactant :- A reactant which is present in lesser number of moles than required as per…

Q: PRACTICE PROBLEMS 1) For the reaction: 4 N,H4 + 2 N2O42)– 6 Nxe + 8 H2O, the theoretical yield of…

Q: In a laboratory experiment 2.00g of carbon monoxide gas yields 3.17g of iodine. What is the percent…

A: Given data contains Mass of CO is 2.00 g. Molar mass of CO is 28 g/mol. The moles of CO is…

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 balanced chemical reaction: 2CH3OH + 302 - 2 + 4H₂0
Use the mass of the following elements
Ic
H
o
12.00 1.00
16.00
What is the percent yield for a process in which 10.4 g CH3OH reacts with 10.1g 0₂ and the actual yield is 10.0g CO2.
Percent

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 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

Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
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 ?
When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
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.
For this reaction, fill in the table with the indicated quantities for the balanced equation. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
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.
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?
Hexamethylenediamine (C6H16N2) is one of the starting materials for the production of nylon. It can be prepared from adipic acid (C6H10O4) by the following overall equation: C6H10O4(l) + 2NH3(g) + 4H2(g) C6H16N2 (l) + 4H2O (l) What is the percent yield for the reaction if 765 g of hexamethylenediamine is made from 1.00 103 g of adipic acid?
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.
A natural brine found in Arkansas has a bromide ion concentration of 5.00 × 10−3 M. If 210. g Cl2 were added to 1.00 × 103 L of the brine, determine the limiting reactant. calculate the theoretical yield of Br2 (d = 3.12 g/mL).
Quicklime, CaO, is formed when calcium hydroxide is heated. Ca(OH)2(s) → CaO(s) + H2O(ℓ) The theoretical yield is 65.5 g but only 36.7 g quicklime I is produced. Calculate the percent yield.
A 0.20 mol sample of magnesium burns in air to form 0.20 mol of solid MgO. What amount (moles) of oxygen (O2) is required for a complete reaction?