Answered: If the theoretical yield of SO2 in the…

If the theoretical yield of SO2 in the reaction is 83.2 grams, and 41.3 grams are actually produced, what is the % yield of SO2? 4 Fes + 7 02 → 2 Fe,03 + 4 SO2

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter5: Chemical Reactions

Section: Chapter Questions

Problem 5.58E

See similar textbooks

Related questions

Q: Aqueous hydrochloric acid (HCI) reacts with solid sodium hydroxide (N2OH) to produce aqueous sodium…

A: The balanced reaction taking place is HCl + NaOH ------> NaCl + H2O Given : mass of HCl taken =…

Q: Methanol has tremendous potential to be used as an alternate fuel. Carbon monoxide gas reacted with…

A: •Here we are producing methanol(CH3OH) by reacting carbon monoxide (CO) with Hydrogen gas(H2). •Here…

Q: Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NAOH) to produce aqueous sodium…

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: The synthesis of maleic acid anhydride (C₄H₂O₃) can be accomplished by reacting benzene (C₆H₆) and…

A: We have, actual yield of maleic acid anhydride = 128.3 g and, percent yield = 72.6 % We…

Q: Certain salts of benzoic acid have been used as food additives for decades. The potassium salt of…

A: "Since you have asked multiple sub-parts, so only three initial sub-parts will be answered as per…

Q: The gaseous hydrocarbon acetylene, C2H2C2H2, used in welders’ torches, burns according to the…

A: The given reaction is as follows: The given mass of acetylene = 26.6 g The actual yield of carbon…

Q: Consider the reaction: 4 Fe + 3 O2 = 2 Fe2O3 If you react 8.00 moles of Fe and produce 3.00…

A: We have given that 4Fe + 3O2 -------> 2Fe2O3 We have given that when 8 mole of Fe react and…

Q: The synthesis of maleic acid anhydride (C„H2O3) can be accomplished by reacting benzene (CHs) and…

A: According to the balanced chemical equation for 100% yield, 2 moles of maleic anhydride requires 2…

Q: If the theoretical yield of the reaction below corresponds to 74.8 gg and the actual yield was 57.4…

A: The percent yield is the ratio of actual yield to theoretical yield, which is expressed as…

Q: Lime, CaO, can be produced in two steps as shown in the equations below. If the percentage yield of…

Q: For the following reaction, 3.69 grams of water are mixed with excess diphosphorus pentoxide. The…

A: What is the theoretical yield of phosphoric acid 13.4grams (2) 85.8percent yield for this…

Q: What is the percent yield for the reaction of nitrogen and hydrogen to produce ammonia, if the…

A: We have the equation for calculating percent yield as follows % yield=Actual yieldTheoretical yield…

Q: 14. Iron metal is used extensively in the manufacture of automobiles. It can be produced by the…

A: we have Fe2O3 + 3CO ------------ 2 Fe + 3 CO2

Q: A sample of calcium metal of mass 2.0 g reacts with excess oxygen. Ca + O2 → CaO You get 2.06 g of…

A: Given Mass of Ca = 2 g actual yield of CaO = 2.06 g

Q: Certain salts of benzoic acid have been used as food additives for decades. The potassium salt of…

A: Given: mass of toluene = 10.750 g mass of KMnO4 = 14.750 g molar mass of toluene = 92.14 g/mol molar…

Q: reaction product is produced in a 76.3% yield. If the actual yield of the isolated product is 31.1…

A: Percentage yield= (actual yield/theoretical yield)*100% Let m=theoretical yield 76.3 =(31.1/m)*100…

Q: For the following reaction, 3.29 grams of oxygen gas are mixed with excess ammonia. The reaction…

A: The ratio of actual yield to the theoretical yield multiply by 100 is known as percentage yield.

Q: For the following reaction, 3.69 grams of water are mixed with excess diphosphorus pentoxide. The…

A: The theoretical yield of phosphoric acid (H3PO4) is calculated as shown below. nH2O=3.69 g18.02…

Q: When heated with sulfuric or phosphoric acid, cyclohexanol, C6H110H, is converted to cyclohexene,…

A: Given mass of cyclohexene = 25 g percent yield = 83℅ molar mass of cyclohexene = 82 g/mol molar mass…

Q: If the theoretical yield of the following reaction is 3.43g of MgO and the actual yield is 2.48g of…

A: Given, Theoretical yield = 3.43 g Actual yield = 2.48 g % yield = ?

Q: In the reaction of 28 g NO,and 18 g H,O by the chemical equation: NO2 (g) + H;O (1) → HNO3 (1) + NO…

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

Q: c) For the equation (NH4)2CO3 → CO2 + H20 + NH3, if 4.01 moles of (NH4)2CO3 reacted, what is the…

A: The theoretical yield seems to be the highest possible quantity of product that can be made from a…

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: A student conducts the following reaction: Fe3O4 + 4 CO ? 3 Fe + 4CO2 If the student starts…

Q: What is a limiting reagent and theoretical yield in grams of NO2 when 10.0 g NH3 react with

A: Given , mass of NH3 = 10.0g. Mass of O2 = 10.0 g. The balance reaction is…

Q: For the following reaction, 5.84 grams of oxygen gas are mixed with excess carbon monoxide. The…

Q: Consider the reaction of solid P₄ and chlorine gas to form gaseous phosphorus trichloride. The…

A: Percent yield of any reaction is given in terms of product as

Q: Consider the synthesis of urea in the process described by the equation: 2 NH3 + CO2 -> CH4N2O+H2O…

Q: 3H2(g)+N2(g)→2NH3(g) 1.86 g H2 is allowed to react with 9.74 g N2, producing 1.69 g NH3. a) What is…

A: Limiting reagent is the reactant that limits the chemical reaction and determines the amount of the…

Q: Consider the reaction: Bry(g) + 3F2(g) - 2BRF3(g) Calculate the theoretical yield (in grams) for…

Q: Lime, CaO, can be produced in two steps as shown in the equations below. If the percentage yield of…

A: Given : Percentage yield of step 1 = 83.5% Percentage yield of step 2 = 71.4%

Q: In preparation of ammonia (NH3), the reaction of 7.2 g of H2 with 75 g of N2 produced 36 g of…

A: identify the % yield of ammonia given data and value 1= 7.2g of hydrogen 2= 75g of Nitrogen 3=…

Q: Balance the equation. What is the limiting reactant when 10.750 g of toluene react with 14.750 g of…

A: (1) The balanced Chemical equation is - C7H8 + 2KMnO4 ---> KC7H5O2 + 2MnO2 + KOH + H2O…

Q: Aqueous sulfuric acid (H, SO 4) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium…

A: 2NaOH + H2SO4 → Na2SO4 + 2H2O 2mol NaOH react with 1 mol H2SO4 to produce 2 mol H2O Molar mass NaOH…

Q: Hexamethylenediamine (C6H16N2) is one of the starting materials for the production of nylon. It can…

A: Adipic acid reacts with ammonia and hydrogen to form hexamethylenediamine and water. The equation…

Q: the reaction starts out with 352 particles of A and 315 particles of B, what is the ideal…

Q: Given the following reaction equation: C4H10 (g) + O2(g) → CO2 (g) + H2O (l) 1) Balance this…

A: the solution is as follows:

Q: For the following reaction, 0.193 moles of sulfur dioxide are mixed with 0.121 moles of water.…

A: The balanced chemical equation is - SO2 + H2O → H2SO3 The limiting reagent is the reagent that is…

Q: 1.14 g H2 is allowed to react with 10.2 g N2 producing 1.08 g NH3 What is the theoretical yield in…

A: The reaction to produce NH3 is as follows: N2+ 3H2 → 2NH3 The mass of H2=1.14 g The mass of…

Q: What is the percent yield of a reaction that produced 15.7 g of AICI3, that has theoretical yield of…

A: Introduction : Percent yield of the reaction can be defined as the percent ratio of actual yield to…

Q: Consider the reaction: 2 SO2(g) + O2(g) → 2 SO3(g) If 6.940 g SO2 is mixed with 17.41 g O2,…

A: The reaction given is 2 SO2(g) + O2(g) → 2 SO3(g) Hence from the above reaction, we can say that 2…

Q: Lime, CaO, can be produced in two steps as shown in the equations below. If the percentage yield of…

Q: Given the reaction below produced 22.95 g of AlCl3 : Al2(CO3)3 + 6 HCl → 2 AlCl3 + 3 H2O + 3 CO2…

Q: For the following reaction, 6.21 grams of butane (C4H10) are mixed with excess oxygen gas. The…

A: Butane reacts with oxygen to form carbon dioxide and water. The equation for the balanced chemical…

Q: For the following reaction, 5.84 grams of oxygen gas are mixed with excess carbon monoxide. The…

Q: If the theoretical yield for a reaction is 100.0 g of a product, and the amount collected when the…

A: Percent yield is defined as measurement in quantity of moles of product formed in chemical reaction…

Q: Determine the limiting reactant and the percent yield of this reaction. How many molecules of…

Q: Hexamethylenediamine (C6H16N2) is one of the starting materials for the production of nylon. It can…

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

If the theoretical yield of SO2 in the reaction is 83.2 grams, and 41.3 grams are
actually produced, what is the % yield of SO2?
4 Fes +7 02 → 2 Fe,03 + 4 SO2
Round to 1 Decimal places!

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

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.
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.
4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g)+3H2O(l)3CO(g)+7H2(g)
Propane, C3H8, is the fuel of choice in a gas barbecue. When burning, the balanced equation is C3H8+5O23CO2+4H2O a What is the limiting reactant in cooking with a gas grill? b If the grill will not light and you know that you have an ample flow of propane to the burner, what is the limiting reactant? c When using a gas grill you can sometimes turn the gas up to the point at which the flame becomes yellow and smokey. In terms of the chemical reaction, what is happening?
Fig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.
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.
Urea is used as a fertilizer because it can react with water to release ammonia, which provides nitrogen to plants. (NH2)2CO(s) + H2O() 2 NH3(aq) + CO2(g) (a) When 300. g urea and 100. g water are combined, calculate the mass of ammonia and the mass of carbon dioxide that form. (b) Calculate the mass of the excess reactant that remains after reaction.
Small quantities of oxygen gas can be generated in the laboratory by the decomposition of hydrogen peroxide. The unbalanced equation for the reaction is H2O2(uz/)-? H2O(/) + O2(g) Calculate the mass of oxygen produced when 10.00 g of hydrogen peroxide decomposes.
For each of the following balanced reactions, calculate how many moles of each product would be produced by complete conversion of 0.50 mole of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. msp;2H2O(l)2H2O(l)+O2(g) msp;2KClO3(s)2KCl(s)+3O2(g) msp;2Al(s)+6HCl(aq)2AlCl3(aq)+3H2(g) msp;C3H8(g)+5O2(g)3CO2(g)+4H2O(g)
3.105 Nitric acid is often sold and transported as a concentrated 16 M aqueous solution. How many gallons of such a solution would be needed to contain the roughly 2.1109 pounds of HNO3 produced annually in the United States?
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.
4.71 The particulate scale drawing shown depict the products of a reaction between N2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) Identify the limiting reactant, and explain how the pictures allow you to do so.