Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S + 3O2 2SO3 In a particular experiment, the reaction of 1.0 g S with 1.0 g O2 produced 0.80 g of SO3. The % yield in this experiment is __________

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S + 3O2 2SO3 In a particular experiment, the reaction of 1.0 g S with 1.0 g O2 produced 0.80 g of SO3. The % yield in this experiment is __________

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 9RQ: Consider the following mixture of SO2(g) and O2(g). If SO2(g) and O2(g) react to form SO3(g), draw a...

See similar textbooks

Related questions

Q: NH3+O2-->NO+H2O When 40.0 g NH3 and 50.0g O2 are allowed to react, using the theoretical yield of…

A: Given :- NH3 + O2 → NO + H2O (unbalanced chemical reaction) Mass of NH3 = 40.0 g Mass of O2 =…

Q: For the following reaction, 6.27 grams of methane (CH4) are mixed with excess carbon tetrachloride.…

A: Methane reacts with carbon tetrachloride to form dichloromethane. The equation of the balanced…

Q: The following chemical equation, which is unbalanced, shows the reaction for the rusting iron…

Q: Acetic acid (vinegar) is produced industrially by combining methanol with carbon monoxide as…

A: The given reaction is CH3OH + CO → CH3COOH According to this reaction , 1 mol of methanol is…

Q: Limiting and Excess Reactants Show ALL work for the following calculations: la. If you perform the…

Q: Liquid octane CH3CH26CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2…

A: Given the reaction, 2CH3(CH2)6CH3 + 25O2 → 16CO2 + 18H2O weight of octane = 19.4g weight of oxygen =…

Q: Gaseous methane (CH₂) reacts with gaseous oxygen gas (O₂) to produce gaseous carbon dioxide (CO₂)…

Q: 18 g of CH4(g) are reacted with 5.2 g of O2(g) by the following reaction CH4(g) + 2O2(g) -->…

A: Given, mass of CH4 (g) = 18 g mass of O2 (g) = 5.2 g Now, the moles of CH4 (g) and O2…

Q: The most important commercial process for converting Ny from the air into nitrogen-containing…

Q: 2C8H18 (l) + 25O2 (g) --> 16CO2 (g) + 18H2O (g) The above reaction is the reaction for gasoline…

A: This problem can be solves by : We can see that 2 moles of gasoline is producing 16 moles of CO2.…

Q: how many grams of bromobenzene (C6H5Br) are formed

A: Number of moles = mass/molar mass so, mass = moles × molar mass molar mass of benzene = 78.11…

Q: Aqueous sulfuric acid H2SO4 reacts with solid sodium hydroxide NaOH to produce aqueous sodium…

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

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

A: Given : For Octane (C₈H₁₈) Mass = 4.6 g And For Oxygen (O₂) Mass = 6.4 g Find :…

Q: An iron nail rusts when exposed to oxygen. For the following reaction, 3.56 grams of oxygen gas…

A: This question can be solved using law of multiple proportions.

Q: Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and…

A: Mass of methane, CH4 = 0.96 g Mass of Oxygen gas, O2 = 2.6 g Molar mass of methane, CH4 = 16.04 g…

Q: limiting reactant?

Q: CH4 + 2H2O CO2 + 4H2 a How many moles of CH4 is needed to form 6 moles of H2? h. What is the…

A: Given reaction : CH4 + 2 H2O ------> CO2 + 4H2 Data given: Moles of H2 = 6 mol Mass of CH4 =…

Q: Use 1 decimal point for all atomic masses. 82.1 g of Ni3C(s) are reacted with 1.80 g of H2(g) by the…

A: The reaction given is Ni3C(s) + 2H2(g) --> 3Ni(s) + CH4(g) Since mass of Ni3C taken = 82.1 g And…

Q: Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane…

A: Note:-1) 1 metric ton =1000Kg 2)1kg=1000kg 3)Molar mass of propane is 44g/mole 4)% yield = [Actual…

Q: 2Al(s) + 3H2SO4(aq) --> Al2(SO4)3(aq) + 3H2(g) A. Determine the volume (mL) of 15.0 M sulfuric acid…

A: Given: Concentration of H2SO4 = 15.0 M Mass of Al = 45.0 g The balanced equation is: 2Al(s) +…

Q: For the following reaction: Aℓ + Fe2O3 → Aℓ2O3 + Fe If 5.0g of Aℓ is added to…

A: Given, Chemical Reaction : Aℓ + Fe2O3 → Aℓ2O3 + Fe Mass of Al : 5.0 g Mass of Fe2O3 : 7.1 g

Q: how many g of Fe2O3 will you obtain from reacting 14.4 g FeS2 and 13.0 g of O2? When rounding…

Q: (a) Consider the reaction: MnO2 + 4HCl --> MnCl2 + Cl2 + 2H2O If 74.8 g of MnO2 and 48.2 g of…

A: The balanced reaction taking place is given as, => MnO2 + 4 HCl --------> MnCl2 + Cl2 + 2 H2O…

Q: Liquid octane CH3CH26CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and…

A: First convert mass into mole by diving molar mass respectively Then Calculate limiting reagent by…

Q: Determine how much lead iodide (in grams) can be formed from 115g of lead nitrate and 265g of…

A: Limiting reagent is the reagent which is consumed in the chemical reaction completely. It decides…

Q: For the reaction AlCl3 + Na2SO4 --> Al2(SO4)3 + NaCl…

A: Given For the reaction AlCl3 + Na2SO4 --> Al2(SO4)3 + NaCl…

Q: If 10.0g of copper reacts with 40.0g of silver (I) nitrate, determine the limiting reactant and the…

A: The species having tendency to wholly decline or consume in chemical reactions and limits the…

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

A: Given, Aqueous hydrochloric acid (HCl) reacts with solid Sodium hydroxide (NaOH) to produce aqueous…

Q: 3 Cu + 8HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H2O In the above equation how many moles of water can be…

A: Given- Reaction-3 Cu + 8 HNO3 → 3 Cu(NO3)2 + 2 NO + 4 H2O Mass of HNO3 = 138.6 grams To find- Number…

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

A: Given mass of HCl = 2.9 g mass of NaOH = 2.9 g

Q: When reacting 5.00 g of MgCl2 with 15.0 g of AgNO3 , what is the limiting reagent based on the…

A: Limiting reagent is the reagent which is present in less quantity and due to which reaction gets…

Q: Aqueous hydrobromic acid HBr reacts with solid sodium hydroxide NaOH to produce aqueous sodium…

A: First convert mass into mole by diving molar mass respectively Then Calculate limiting reagent by…

Q: For each of the following balanced reactions, suppose exactly 5.00 moles of each reactant are taken.…

Q: Base on the following chemical equation: NH3(g) + F2(g) ---> N2F4(g) + HF(g) 1. How many grams of…

Q: Methyl alcohol (wood alcohol), CH3OH, is produced via the reaction: CO(g) + 2 H2(g ) → CH3OH (1) A.…

A: Welcome to bartleby !

Q: Benzene (C6H6) reacts with bromine (Br2)to produce bromobenzene (C6H5Br) according to the following…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: For the following reaction: N2(g) + 3 H2(g) -----> 2 NH3(g) a. Determine the…

A: The reaction's yield derived using stoichiometry and limiting reactant's amount is termed as…

Q: Under certain circumstances, carbon dioxide, CO2(g)CO2(g), can be made to react with hydrogen gas,…

A: 1) Since from the balanced reaction we can see, 1 moles of CO2 reacts to form 1 mole of methane i.e…

Q: When the following equation is properly balanced, what are the coefficients for C6H6(l), O2(g),…

A: The question is about writing the coefficients of the given Chemical equation -

Q: When iron and steam react at high temperatures, the following reaction takes place. Fe(s) + H2O(g)…

Q: In a particular experiment 0.0039 moles of AgNO3 is added to 0.001875 NH4Cl and 0.156g of AgCl are…

A: The balanced reaction taking place is given as, => AgNO3 (aq) + NH4Cl (aq) ------> AgCl (s) +…

Q: When 30.0 g of MgCl2 and 30.0 g of Na2CO3 are reacted MgCl2 + NazCO3 MgCO3 + 2 NaCI the limiting…

Q: If 25.8g of P4 is allowed to react with 19.2g of S8, which is the limiting reactant. P4+S8 -> P4S3

A: The limiting reagent is the reagent that is used up completely. This stops the reaction and no…

Q: NaOH + H3PO4 --> Na3PO4 + H2O In the unbalanced reaction above if 39.7g NaOH and 55.9g H3PO4 are…

A: Moles are defined as the mass-to-molar mass ratio. It is represented by n. The number of moles…

Q: l2O5+5CO 5CO2+l2 80.0 g of iodine (V) oxide reacts with 28.0 g of carbon monoxide what is the…

Q: Iodine reacts with antimony in the following manner 2Sb(s)+3I(s) ---> 2SbI3(s) in an…

Q: For the reaction below, 61.5 g of sulfur trioxide reacts with 11.2 g of water to produce 54.9 g of…

A: The reaction given is SO3 + H2O -----> H2SO4 Given : mass of SO3 taken = 61.5 g mass of H2O…

Q: Ethanol (CH3CH₂OH), the intoxicant in alcoholic beverages, is also used to make other organic…

A: In concentrated sulfuric acid,ethanol forms diethyl ether and water according to the following…

Question

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant:

2S + 3O2 2SO3
In a particular experiment, the reaction of 1.0 g S with 1.0 g O2 produced 0.80 g of SO3. The %

yield in this experiment is __________.

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 with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
Cyanogen gas, C2N2, has been found in the gases of outer space. It can react with fluorine to form carbon tetrafluoride and nitrogen trifluoride. C2N2(g)+7F2(g)2CF4(g)+2NF3(g)(a) How many moles of fluorine react with 1.37 mol of cyanogen? (b) How many moles of CF4 are obtained from 13.75 mol of fluorine? (c) How many moles of cyanogen are required to produce 0.8974 mol of NF3? (d) How many moles of fluorine will yield 4.981 mol of nitrogen trifluoride?
Chlorine and fluorine react to form gaseous chlorine trifluoride. Initially, 1.75 mol of chlorine and 3.68 mol of fluorine are combined. (Assume 100% yield for the reaction.) (a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) What is the theoretical yield of chlorine trifluoride in moles? (d) How many moles of excess reactant remain after reaction is complete.
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?
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.
Ammonia gas can be prepared by the following reaction: CaO(s) + 2 NH4Cl(s) 2 NH3(g) + H2O(g) + CaCl2(s) If 112 g of CaO and 224 g of NH4Cl are mixed, the theoretical yield of NH3 is 68.0 g (Study Question 12). If only 16.3 g of NH3 is actually obtained, what is its percent yield?
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.
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?
For each of the following balanced equations, indicate how many moles of the product could be produced by complete reaction of 1.00 g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. msp;NH3(g)+HCl(g)NH4Cl(s) msp;CaO(s)+CO2(g)CaCO3(s) msp;4Na(s)+O2(g)2Na2O(s) msp;2P(s)+3Cl2(g)2PCl3(l)
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.
Consider the equation: 2A+B5C. If 10.0 g of A reacts with 5.00 g of B. how is the limiting reactant determined? Choose the best answer and explain. l type='a'> Choose the reactant with the smallest coefficient in the balanced chemical equation. So in this case, the limiting reactant is B. Choose the reactant with the smallest mass given. So in this case, the limiting reactant is The mass of each reactant must be converted to moles and then compared to the ratios in the balanced chemical equation. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must he converted to moles first. The reactant with the fewest moles present is the limiting reactant. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must be divided by their coefficients in the balanced chemical equation, and the smallest number present is the limiting reactant. So in this case, there is no limiting reactant because A and B arc used up perfectly.
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)