Question 33In a chemical equation, AsF3 + Cl4 - AsCl3 + CCI2F2, the theoretical yield of CCI2F2 was calculated to be 203 g. If 151 g of CCI2F2 product was obtained, what was the percent yieldof this reaction?O 15.1%O 74.4%O 0.744%O 20.3%

The given chemical reaction is: AsF3 + CCl4 → AsCl3 + CCl2F2 The given information is: Theoretical…

estion 33 In a chemical equation, ASF3 + CCl4 - AsCl3 + CCl2F2, the theoretical yield of CCI2F2 was calculated to be 203 g. If 151 g of CCl2F2 product was obtained, what was the percent yield of this reaction? O 15.1% O 74.4% O 0.744% O 20.3%

estion 33 In a chemical equation, ASF3 + CCl4 - AsCl3 + CCl2F2, the theoretical yield of CCI2F2 was calculated to be 203 g. If 151 g of CCl2F2 product was obtained, what was the percent yield of this reaction? O 15.1% O 74.4% O 0.744% O 20.3%

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: Given the following equation: 2KClO3=2KCl+3O2 How many moles of KClO3 are needed to produce 130.0 g…

A: Potassium chlorate decomposes into potassium chloride and oxygen gas. The equation for the balanced…

Q: True or false to calculate the percent yield of a reaction, the correct formula is percent yield =…

A: Percent yield of a chemical reaction represents the efficiency of an experiment, procedure and…

Q: How many grams of KCIO3 are needed to produce 6.00 g of O₂? The percent yield for the reaction below…

Q: How many moles of NO₂ would be produced from 3.8 mol of O₂ in the reaction below assuming the…

Q: When HgO is heated, it decomposes into elemental mercury and molecular oxygen. If 10.0 g of Hg is…

A: Given :- HgO → Hg + O2 Actual yield of Hg = 10.0 g Mass of HgO decompose = 20.0 g To calculate…

Q: How many grams of NH3 are expected to be produced from the reaction of 58.7 g of N2 with excess H2…

A: N2 (g) + 3H2 (g) -------> 2NH3 (g) Moles of N2 , nN2 = weight ÷ molar mass nN2 = 58.7 ÷ 28 nN2 =…

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: How many moles of NO₂ would be produced from 4.7 mol of O₂ in the reaction below assuming the…

A: 2NO + O2 ....> 2NO2 Moles of O2 = 4.7 mol Percent yield of NO2 = 57.0%

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: What is the mass in grams of H2 that can be formed from 44.8 grams of NH3 in the following reaction?…

A: The given reaction shows that two moles of ammonia reacts to form three moles of hydrogen and one…

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

A: Percent yield = actual yield / theoretical yield x 100%.

Q: A 7.50 g sample of hydrogen peroxide decomposes according to the reaction b 2 H2O2(aq) - 2 H20(1) +…

Q: What is the percent yield of water when you have 3.8 g H₂O produced from the reaction of 9.0 g CH3OH…

A: The mass of water that produced= 3.8 gThe mass of methanol reacts = 9.0 gThe mass of oxygen reacted…

Q: Only 4.00 g of O 2 were actually produced by the reaction below; this represents a 65.0% yield. How…

Q: How many moles of NO₂ would be produced from 6.2 mol of O₂ in the reaction below assuming the…

A: Given percent yield = 57.0 % => Actual YieldTheoretical Yield*100 = 57.0 The question asks to…

Q: Consider the combination reaction: 2 Al(s) + 3 Br2(1) 2 AIBr3(s) ----> Suppose the actual yield of…

A: We have to predict the theoretical yield.

Q: Fernando is doing his pre-lab homework for Chemistry. He is asked to predict how many grams of CO2…

A: Actual yield = 30.65 g Theoretical yield = 46.0 g

Q: When 50.0 g of Fe was burned in the presence of excess oxygen, 27.0 g of Fe₂O3 was produced. If the…

Q: Calculate the percent yield for water.

A: Number of moles = mass/molar mass Molar mass of WO3 is 231.838 g/mol Percent yield = (actual…

Q: Given the following equation: 2 KClO3 → 2 KCl + 3 O2 How many grams of O2 are produced when 56.00…

A: According to Law of conservation of mass, we balanced the chemical reaction. In any chemical…

Q: Consider the following unbalanced reaction: D4(s) +X2(g) -> DX3(g) Determine the amount of X2 (in…

A: Percent yield=actual yieldtheoretical yield×100 Actual yield is the amount of product formed from…

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: If 15.2 g N2 and 1.65 g H2 react to produce 1.33 g NH3, what is the percent yield of the reaction?…

Q: The combustion of liquid ethanol (C2H5OH) produces carbon dioxide and water. After 4.62 mL of…

A: The balanced reaction of ethanol combustion is given as - C2H5OH + 3O2 -----> 2CO2 + 3H2O It…

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: What is the mass in grams of H₂ that can be formed from 43.6 grams of NH₃ in the following reaction?…

A: Molar mass of NH3 = Atomic mass of N + H x 3 = 14 g/mol + 1 g/mol x 3…

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

Q: If 6.8 g of a hydrocarbon that is 83.2% C by mass is burned with O2 to make CO2 and H2O, what mass…

Q: Consider the following balanced reaction. What mass (in g) of CO2 (44.01g/mol) can be formed from…

Q: Complete combustion of a 1.448 g sample of a hydrocarbon (only carbon and hydrogen present),…

A: Given -> Weight of hydrocarbon = 1.448 gm Weight of CO2 = 3.128 gm Weight of H2O = 1.121 gm

Q: What mass of CO2 is produced when 100.0 g of Fe is produced? 118.2 g…

A: 1) Mass of CO2 produced = 118.2 g2) Mass of Fe produced = 69.94gExplanation:The balanced reaction…

Q: When 12.0 g of carbon is burned in oxygen during an experiment, only 40.4 g of carbon dioxide was…

A: Weight of 1 mole of compound is called the molar mass of that compound.

Q: Combustion of 8.45 mg of an unknown substance yields 14.0 mg CO2 and 7.08 mg H20. The unknown…

A: We have to calculate the % of each element in substance.

Q: State which amount of product is the Theoretical Yield. FeSO4 + Potassium phosphate à…

A: The reaction given is, => FeSO4 + Potassium phosphate→ Iron (II) phosphate + K2SO4 => FeSO4…

Q: Given that the reaction below has a yield of 84.36%, If you needed to create 26.29 g of SbCl3…

Q: Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When…

Q: Combining 0.266 mol Fe,O, with excess carbon produced 20.0 g Fe. Fe, O, + 3 C → 2 Fe + 3 CO What is…

A: Given,Moles of Fe2O3 = 0.266mol.Mass of Fe produced = 20.0g.The actual yield of iron in moles is…

Q: How many grams of NO are required to produce 145 g of N₂ in the following reaction? 4NH3 + 6NO →→…

A: This can be explained as:

Q: Each step in the following process has a yield of 80.0%. CH4+4Cl2⟶CCl4+4HCl CCl4+2HF⟶CCl2F2+2HCl The…

A: A question is based on general chemistry, which is to be accomplished.

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

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

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

If 14.0 g of C₂H4 react completely to form 7.84 g of water, as shown below, the percent yield in the reaction is 2C₂H₂ + 60₂ 4 CO₂ + 4H₂O O 43.6% O 56.0 % 64.7% 87.1%
What is a correct mole ratio for this reaction? 2 KCIO, -->2 KCl +30₂ O 3 mol KCIO: 2 mol O₂ O 2 mol KCIO,: 3 mol O₂ Othey are all correcti 01 mol KCIO,: 1 mol O₂
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 +.
How many moles of NO₂ would be produced from 4.5 mol of O₂ in the reaction below assuming the reaction has a 57.0% yield? 2 NO (g) + O₂ (g) → 2 NO₂ (g)
Complete combustion of 3.703.70 g of a hydrocarbon produced 12.012.0 g of CO2 and 3.703.70 g of H2O. What is the empirical formula for the hydrocarbon
According to the following reaction, how many grams of hydrofluoric acid will be formed upon the complete reaction of 26.4 grams of water with excess silicon tetrafluoride? silicon tetrafluoride (s) + water (I) --> hydrofluoric acid (aq) + silicon dioxide (s) O58.6g O 2.9g O 14.7g 20.2g
22.0 g of CO2 gas and 9.01 g of H2O gas are formed from combustion of an unknown hydrocarbon (containing only hydrogen and carbon) in the presence of O2 gas. The molar mass of the gas is 84.2 g/mol. What is its molecular formula?
When 12.0 g of carbon is burned in oxygen during an experiment, only 39.8 g of carbon dioxide was collected. What is the percentage yield? C + O2 -> CO2
What is the percent yield if 28.16 g of CO2 is collected from a reaction with a theoretical yield of 225.3 g of CO2? 20.00% 50.00% O 25.00% O 12.50%
A student was able to detect a mass increase of 0.500 grams during the reaction between Mg and O2. Oxygen was present in excess and the starting mass of Mg was 1.00 g. What is the percent yield of the reaction? O 50.0% O 90.9% O 150.% O 66.7%
When 5.0 g of propane are reacted with O2, carbon dioxide and water are produced. How many grams of H2O can be produced by the complete reaction of those 5.0 g of propane with excess oxygen? 20 g 1.1 g 8.2 g 0.45 g 2.04 g
The theoretical yield for CaO in the reaction above is 18.9 g. What is the percent yield if 16.1 g CaO is actually produced?