Answered: The theoretical yield for a reaction…

The theoretical yield for a reaction was 150 grams and actually 126 grams of the product were made, what is the percent yield?

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

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 35Q: What is the theoretical yield for a reaction, and how does this quantity depend on the limiting...

See similar textbooks

Related questions

Q: The theoretical yield of aluminum is 1.16 moles. If only 1.03 moles of aluminum were collected, what…

A: Given, Theoretical yield = 1.16 moles Actual yield = 1.03 moles % yield = ?

Q: The reaction of iron (III) oxide reacts with carbon to produce iron metal and carbon dioxide. What…

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

A: The given data contains, Theoretical yield = 0.118 g. Actual yield = 0.104 g.

Q: A 0.216 g piece of solid magnesium reacts with gaseous oxygen from the atmosphere to form solid…

A: mass of magnesium (Mg) reacts = 0.216 g Actual yield of magnesium oxide (MgO) = 0.234 g Percent…

Q: The percent yield of a reaction is 32.4%. If an experimental value of 221.42g of product is…

Q: In a certain experiment, 40.0g KClO3 is heated until it completely decomposes. What is the…

Q: A 0.156g piece of solid aluminum reacts with gaseous from the atmosphere to form solid aluminum…

A: 4Al + 3O2 ------------> 2Al2O3 Molecular mass of Al2O3 = 102g

Q: A 0.256 g piece of solid magnesium reacts with gaseous oxygen from the atmosphere to form solid…

Q: Ca(s) + 2HCI(aq) CaCl2(aq) + H2(g) If 1.00 g of Ca reacts with 0.850 g HCl and 1.21 g CaCl, are…

A: This problem can be done via mole mole analysis.

Q: The percent yield for a given reaction is 47%. If the theoretical amount is predicted to be 5.29 g,…

A: Formula for calculating percent yield: Percent yield = 100 x Actual yield/Theoretical yield

Q: The theoretical yield for a given compound in a reaction is 21.3 g. The actual yield is 8.72 g.…

Q: A reaction yields 6.26 g of a product. What is the percent yield if the theoretical yield is 18.81…

A: Given, actual yield = 6.26 g theoretical yield = 18.81 g percent yield = ?

Q: If the percent yield for a reaction is 100% and the theoretical yield is 88 g. What is the actual…

A: Actual yield is defined as quantity of a product received from a chemical reaction.

Q: the percient yield for a difficult reaction to be studied was likely to be only 23% of the…

A: According to given data, the actual yield for a reaction to be studied was likely to be 23% of the…

Q: If the theoretical yield of a reaction is 0.102 gg and the actual yield is 9.40×10−2 gg , what is…

Q: The percent yield for a given reaction is 75%. If the theoretical amount is predicted to be 3.58g,…

A: Percent yield of the reaction is equal to the ratio of actual yield and theoretical yield multiplied…

Q: A reaction has a theoretical yield of 55.8 g. When the reaction is carried out, 37.2 g of the…

A: Percent yield is the percent ratio of actual yield to the theoretical yield. It is calculated to be…

Q: For the following reaction, 5.06 grams of bromine are mixed with excess chlorine gas . The reaction…

Q: The theoretical yield of a reaction is 75.0 grams of product and the actual yield is 42.0 g. what is…

A: Given as The theoretical yield of a reaction is 75.0 gram and actual yield is 42.0 g % yield has to…

Q: The percent yield for a given reaction is 60%. If the theoretical amount is predicted to be 8.33 g,…

A: Given: Percent yield= 60% Theoretical yield= 8.33 g

Q: For a given reaction, the theoretical yield for a reaction was 34.7 grams while 29.6 grams of the…

A: Answer

Q: what is the percent yield?

A: The ratio between the actual yield and the theoretical yield multiply by 100 is known as percent…

Q: For the following reaction, 4.44 grams of calcium hydroxide are mixed with excess sulfuric acid. The…

A: calculate the theoretical yield and percentage yield from the given data.

Q: A chemical reaction producing the imaginary chemical nocebo has a percent yield of 74.5% if you…

A: Given: For compound nocebo: Percentage yield = 72.5% Actual yield required = 43.0g To find:…

Q: If the theoretical yield of a reaction is 23.6 g and the actual yield is 17.4 g , what is the…

A: • The values provided in the question are:- i) Theoretical yield of a reaction, T = 23.6 g…

Q: expected

A: Dear student I have given answer to your question in the image format.

Q: In a reaction to produce sulfuric acid, the theoretical yield is 300. g. What is the percent yield…

A: Therotical yield of H2SO4 = 300 g Actual yield of H2SO4= 111.4 g

Q: The actual yield of one of the reactions in 43.5g. What was theoretical yield in the laboratory if…

Q: The theoretical yield of a reaction is 75.0 grams of product and the actual yield is 42.0 grams.…

A: THEORETICAL yield = 75.0 g actual yield = 42.0 g % yield = ?

Q: The theoritical yeild of a certain compound according to a chemical reaction is 127 g. The percent…

A: Theoretical yield = 127 g percent yield = 82.0% Percent Yield = Actual yieldTheoretical…

Q: A 0.251 g piece of solid aluminum reacts with gaseous oxygen from the atmosphere to form solid…

A: Given: Mass of Al = 0.251 g Mass of Al2O3 (actual yield) = 0.204 g Molar mass of Al = 26.98 g/mol…

Q: For the following reaction, 272 grams of potassium hydrogen sulfate are allowed to react with 56.1…

A: The limiting reagent is that reactant which is completely consumed during the reaction.

Q: In a reaction to produce ammonia, the theoretical yield is 420.0 g. What is the percent yield if the…

A: Percent yield of the reaction is equal to the ratio of actual yield and theoretical yield multiplied…

Q: If the theoretical yield of a reaction is 22.6 gg and the actual yield is 19.9 gg , what is the…

A: Theoretical yield = 22.6 g Actual yield = 19.9 g The percentage yield is given by: % yield = Actual…

Q: A 0.206 g piece of solid magnesium reacts with gaseous oxygen from the atmosphere to form solid…

A: Answer: Oxidation reaction of Mg is shown below: 2Mg(s)+O2(g)→2MgO(s)

Q: 91.30 g of Propane reacts with Oxygen to produce Carbon Dioxide and Water. If 250.3 g of Carbon…

A: The above given reaction is a combustion reaction of propane which can be written as - C3H8 + 5O2…

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

The theoretical yield for a reaction was 150 grams and actually 126 grams of the product were made, what is the percent yield?

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

A yield of 3.00gKClO4 is obtained from the (unbalanced)reaction KClO3KClO4+KCl when 4.00 g of the reactant is used. What is the percentageyield of the reaction?
For the chemical reaction C3H8O2+4O23CO2+4H2O how many product molecules are formed when nine C3H8O2 molecules react?
Calculate the amounts of reactants needed in a chemical reaction to produce a specified amount of product.
What is the theoretical yield for a reaction, and how does this quantity depend on the limiting reactant?
Sulfur dioxide gas reacts with sodium hydroxide to form sodium sulfite and water. The unbalanced chemical equation for this reaction is given below: SO2(g)+NaOH(s)Na2SO3(s)+H2O(l) Assuming you react 38.3 g sulfur dioxide with 32.8 g sodium hydroxide and assuming that the reaction goes to completion, calculate the mass of each product formed.
In a blast furnace at high temperature, iron(III) oxide in ore reacts with carbon monoxide to produce metallic iron and carbon dioxide. The liquid iron produced is cooled and weighed. The reaction is run repeatedly with the same initial mass of iron(III) oxide, 19.0 g, but differing initial masses of carbon monoxide. The masses of iron obtained arc shown in this graph. (a) Write the balanced chemical equation for this reaction. (b) Calculate the mass of CO required to react completely with 19.0 g iron(III) oxide. (c) Calculate the mass of carbon dioxide produced when the reaction converts 10.0 g iron(III) oxide completely to products. (d) From the graph, determine which reactant is limiting when less than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (e) From the graph, determine which reactant is limiting when more than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (f) Calculate the percent yield if 24.0 g iron(III) oxide reacted with 20.0 g carbon monoxide to produce 15.9 g metallic iron. (g) Calculate the minimum mass of additional limiting reactant required to react with all of the excess of nonlimiting reactant from part (f).
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?
Consider a reaction represented by the following balanced equation :math>2A+3BC+4D u find that it requires equal masses of A and B so that there are no reactants left over. Which of the following is true? Justify your choice. l type='a'> The molar mass of A must be greater than the molar mass of B. i>The molar mass of A must be less than the molar mass of B. i>The molar mass of A must be the same as the molar mass of B.
The text explains that one reason why the actual yield for a reaction may be less than the theoretical yield is side reactions. Suggest some other reasons why the percent yield for a reaction might not be 100%.
If baking soda (sodium hydrogen carbonate) is heated strongly, the following reaction occurs: :math>2NaHCO3(s)Na2CO3(s)+H2O(g)+CO2(g) lculate the mass of sodium carbonate that will remain if a 1.52-g sample of sodium hydrogen carbonate is heated.
The simplest example of the hydrogenation of a carbon-carbon double bond is the reaction between ethene and hydrogen in the presence of nickel: CH2=CH2+H2NiCH3CH3. When 5.20g of ethene react with excess hydrogen gas, the reaction yields 4.75g of ethane. What is the percentage yield for this reaction?
Classify each of the following statements as true or false: a Coefficients in a chemical equation express the molar proportions among both reactants and products. b A stoichiometry problem can be solved with an unbalanced equation. c In solving a stoichiometry problem, the change from quantity of given substance to quantity of wanted substance is based on masses. d Percentage yield is actual yield expressed as a percentage of ideal yield. e The quantity of product of any reaction can be calculated only through the moles of the limiting reactant. f rH is positive for an endothermic reaction and negative for an exothermic reaction.