6. Discuss some possible experimental reasons the calculated percent yield of reactions often less to 100% and even occasionally more than 100%. What does a percent yield more than 100% indicate?

The percentage yield is defined as the percentage calculated of the ratio of the actual yield with…

Answered: 6. Discuss some possible experimental…

6. Discuss some possible experimental reasons the calculated percent yield of reactions of often less to 100% and even occasionally more that 100%. What does a percent yield more than 100% indicate?

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: 6. Discuss some possible experimental reasons the calculated percent yield of reactions of often…

A: percent yield = [Actual yield / theoretical yield] x 100Reasons as to why calculated percent yield…

Q: Is the following statement true or false? If you think the statement is flase, rewrite it to make it…

A: The statement given is "The compound or element that is greater in terms of the molar amount is the…

Q: Use the following Unbalanced reaction and the information about starting material to determine the…

Q: In one experiment 6.50 grams of salicylic acid is reacted with excess acetic anhydride. The reaction…

A: % yield = 100 x Obtained amount of product/Calculated amount of product

Q: If 2.88 moles of AlPO4 were needed for a reaction what mass of AlPO4 would need to be measured out

A: The moles of AlPO4 is = 2.88 moles The mass of AlPO4 in grams is =?

Q: In an experiment, you obtain apercent yield of product of 108%. Is such a percent yieldpossible?…

A: Percentage Yield = = (actual yield÷theoretical yield)×100 Theoretical yield is…

Q: limiting reactant= HCI 525g. HCI moles:

A: Number of moles = Mass of the substanceMolar mass of the substance

Q: -> Naz0(s) _CO2(g) H2O(g) Theoretical yield (grams) of NazO: Percent yield (Run 1) =

A: In the given question we have to calculate the theoretical yield of the product formed by the…

Q: Consider the reaction of Fe2O3 with Al to form Al2O3 and Fe. If 4.27 g Al is reacted with excess…

A: Given that,Mass of Al = 4.27 gThe molar mass of Al = Mass of = 6.24 g = Actual yieldThe molar mass…

Q: For this reaction, 14.7 g phosphorus (P4) reacts with 38.8 g chlorine gas. phosphorus (P4) (s) +…

A: Given :Reaction: phosphorus (P4) (s) + chlorine (g) → phosphorus trichloride (l)Mass of phosphorus…

Q: 2D.) Calculate the percent yield if your actual yield was 38.0g of ZnS. Zn + S -> ZnS Zn = 50.0g…

A: Given: Actual yield of ZnS= 38.0g Mass of Zn= 50.0 g Mass of S= 60.0 g The balanced equation is

Q: In this reaction: Mg (s) + I2 (s) Mgl2 (s), if 10.0 g of Mg reacts with 60.0 g of l2, and 53.30 g of…

A: The balanced reaction taking place is given as, => Mg (s) + I2 (s) → MgI2 (s) Given: Mass of Mg…

Q: Example 2: When 40.0 grams of magnesium is placed in an excess of nitric acid, 1.7 grams of hydrogen…

A: Given: Mass of Mg = 40 g Mass of H2 = 1.7 g Standard data: The molar mass of Mg = 24.305 g/mol…

Q: 3.Use the following Unbalanced reaction and the information about starting material to determine the…

Q: A reaction vessel for synthesizing ammonia by reacting nitrogen and hydrogen is charged with 5.04 kg…

A: Given, 5.04 kg of H2 reacts with excess N2 Actual yield of NH3 = 23.2 kg

Q: Sodium borohydride () is prepared by reacting sodium hydride () with gaseous diborane (). In an…

Q: What is the max CaCO3 produced?

Q: 3. If the theoretical yield of a reaction is 0.118 g and the actual yield is 0.104 g, what is the…

A: Theoretical yield = 0.118 g Actual yield = 0.104 g Percent yield = ?

Q: 5.- If 154 g of Al react with 801 g of Fe2O3 to produce Al2O3, and Fe A) Write the balanced equation…

A: A) Balanced equation:B) To find the limiting reactant, we need to calculate the moles of each…

Q: Although xenon is a "noble gas," it reacts with fluorine and oxygen. When xenon gas reacts with F2…

A: Percentile yield is defined as the ratio of actual yield by theoretical yield multiplied by 100.…

Q: -What are two possible reasons why percentage yield is different from 100%

A: There is a theoretical or the stochiometric yield. This yield is calculated using the reaction…

Q: Treatment of Data Mole amount of Na2Cl3 - Moles Na2CO3 = Mole amount of CaCl2- Moles of CaCl2 =…

A: All the details are explained in handwritten solution. Molarity = moles / Volume (L) Moles = mass /…

Q: When hydrogen chloride reacts with magnesium, magnesium chloride and hydrogen gas are formed. How…

A: Given, moles of Mg = 0.4155 mol moles of HCl = 0.7131 mol Theoretical yield of H2 gas = 0.7188 g…

Q: [References] TUTOR Percent Yield Consider this reaction, which occurs in the atmosphere and…

Q: chiometry 5. Lead(III) sulfide reacts with ealcium chloride to produce lead(III) chloride and…

A: Moles of calcium chloride = 0.500 moles Mass of lead chloride = ?

Q: if 10.00 g of iron metal is reacted with 14.5 g of Cla gas, how many grams of ferric chloride (FeCI)…

A: The balanced chemical equation for the reaction between iron metal (Fe) and chlorine gas (Cl2) to…

Q: what is the percent yield?

A: Given :- theoretical yield = 9.4 g actual yield = 1.2 g To calculate :- percent…

Q: Use the following Unbalanced reaction to determine the percent yield of the reactions. For your…

A: Given Mass of Na2SO3 = 41.5 g Molar mass of Na2SO3 = 126.043 g/mole Moles of Na2SO3 = Mass of…

Q: A 3.82 g sample of magnesium nitride is reacted with 7.73 g of water:…

Q: what is the percent yield?

A: Given :- Actual yield of MgO = 2.48 g Theoretical yield of MgO = 4.13 g To calculate :- Percent…

Q: (Mass of crucible and cover is 43.92 g. The mass of crucible, cover, and magnesium is 44.62g. Mass…

Q: Liquid octane CH3CH26CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide…

A: moles of octane = mass/ molecular mass = 2.3/114 = 0.0202 moles of oxygen = 3.2 / 32 = 0.1 Since…

Q: According to the following reaction, how many grams of carbon dioxide will be formed upon the…

A: Given: The mass of oxygen gas is 21.6 g. The reaction between carbon monoxide and oxygen gas to form…

Q: Use the References to access important values if needed for this question. For the following…

A: Given : reactions

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

6. Discuss some possible experimental reasons the calculated percent yield of reactions often less to 100% and even occasionally more than 100%. What does a percent yield more than 100% indicate?

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

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

Cn.
Do not give handwriting solution. Determine the percent yield to two decimal places if 5.53 g of alum are synthesized using 0.43 g of aluminum. (MM Al = 26.98 g/mol; MM alum = 474.38 g/mol)
Chemical Reactions Percent yield of chemical reactions FIGUqcNzzFUDO... 1/3 Julianna Aqueous sulfuric acid (H2SO4) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium sulfate (Na2SO4) and liquid water (H2O). If 9.60 g of water is produced from the reaction of 66.7 g of sulfuric acid and 24.5 g of sodium hydroxide, calculate the percent yield of water. Round your answer to 3 significant figures. % Explanation Check MacBook Air 2024 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility ola Ar
Iron reacts with oxygen at high temperatures to form iron(III) oxide. 4 Fe(s) + 30,(g) 2 Fe,0,(s) Suppose 17.2 g of iron (Fe) is reacted with 16.6 g of oxygen (0,). Select the limiting reagent. O2 Fe O Fe,O, Calculate the theoretical yield of iron(II) oxide (Fe, O,). 3 ald
3.Which is NOT described by the coefficients in a chemical reaction? a.Grams b.Atoms c.Molecules d.Moles
A) Determine the molecular formula of X (the starting reagent) B) Write a balanced equation for this reaction C) Determine the theoretical mass of the CO2 produced if 0.2 mol of O2 is completely consumed D) If the combustion reaction produced is 3.0g of CO2, determine its percentage yield
Given the equation C4H6 + 2HBr ---> C4H8Br2 Calculate the moles of C4H8Br2 produced when 1.5 nole of HBr is mixed with 0.50 mole C4H6
Suppose 65.0 g of K(s) reacts with 25.0 g oxygen gas to produce 54.7 g of potassium oxide. WHat is the % yield. (In class we got 70.0%). When solving could you go over in this problem by teaching me what the actual yield, theorictical yield, and percent yield are and how to find each one of those. It really confuses me which one is which and how to solve for each of them.
mass of Fe: If the actual experimental yield for Fe is 8.29 g, what is the percent yield of Fe? percent yield: %
1) The Law of Conservation of Mass states that the total mass, in an open system, does not change as the result of reactions between its parts. True False 2) The deviation from the theoretical yield to the actual yield is called the percent yield. True False
What does the percent yield mean in describing chemical reactions and why is it not exactly 100%?
Hi! I need help with these limiting reactants questions from my Chem class please