19. When 0.75 moles chromium(III) oxide reacts with 2.5 moles hydrogen sulfide (H2S) gas, chromium(III) sulfide and water were formed. What is the percent yield of Cr2S3 if 125 grams of it was obtained? MW: Cr2S3 = 200.19g/mol Cr2O3(s) + 3H2S(g) -> Cr2S3(s) + 3H2O()

19. When 0.75 moles chromium(III) oxide reacts with 2.5 moles hydrogen sulfide (H2S) gas, chromium(III) sulfide and water were formed. What is the percent yield of Cr2S3 if 125 grams of it was obtained? MW: Cr2S3 = 200.19g/mol Cr2O3(s) + 3H2S(g) -> Cr2S3(s) + 3H2O()

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: Ethyl alcohol can be converted to diethyl by the reaction 2C2H5OH -(arrow to the right)…

A: Mass of ethyl alcohol = 65.3 gMolar mass of ethyl alcohol = 46.07 g/molActual yield of diethyl ether…

Q: Determine the theoretical yield of H 2S (in moles) if 18 mol Al 2S 3 and 18 mol H 2O are reacted…

A: Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. The equation for…

Q: For the reaction shown, calculate how many grams of oxygenform when each quantity of reactant…

A: Note: Since you have posted a question with multiple subparts, we will solve the first three…

Q: Si(s) + 2C12(g) -> SiCI.(0) In one reaction, 0.507 mole of SiCI4 is produced. What mass (grams) of…

Q: Ca(OH)2 (s) + H₂S(g) →→→ CaS(s) + 2H₂O(1) In the reaction above, calcium hydroxide and hydrogen…

A: As we know limiting reactant is the one that is completely reacts in the reaction and the excess…

Q: How many mililiters of O2 are consuked in the complete combustion of a sample of hexane, C6H14, if…

A: The balanced chemical reaction is given as follows: 2C6H14(g)+19O2(g)→12CO2(g)+14H2O(g) The volume…

Q: Consider the reaction C6H1206(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(1). The density of carbon dioxide is…

A: Since mass = density X volume Given : density of CO2 = 1.98 g/L And volume of CO2 = 6.66 L hence…

Q: STARTING AMOUNT X Determine the mass in grams of CO, that are produced by the complete reaction of…

A: This question belongs to Mole concept. Given Mass of Toluene = 0.05090g We know that Molar mass of…

Q: A reaction mixture of 18.215g Na2CO3 and 10.938g HCl react according to the following balanced…

A: The mole ratio between HCl and Na2CO3 is 2 : 1 . First, identify the limiting reactant, Moles…

Q: A mixture of 4.41 g propane (C_{3}*H_{8}) and 6.40 g of oxygen (O_{2}) is ignited . What reactant is…

A: Answer: excess reactant - propane(C3H8) Carbon dioxide (CO2) formed = 5.28 g , Water (H2O) formed =…

Q: 100.00 molecules of H2 and 40.00 molecules of O2 react, how many molecules of H2O can be produced in…

A: In a balanced chemical equation, stoichiometry is utilized to calculate the amount of products…

Q: When 46.19 g NH3 reacts by the following balanced equation, 27.98 H₂O are formed. 4NH3(g) +502(g)…

A: Step 1: Given the information.When 46.19 g NH3 reacts with the following balanced equation, 27.98 g…

Q: Dihydrogen monosulfide reacts with sulfur dioxide according to the balanced equation: 2 H2S( g) +…

A: Dihydrogen monosulfide reacts with sulfur dioxide according to the balanced equation: 2 H2S( g) +…

Q: The following equation represents the combustion reaction of octane (C8H18), which is the primary…

A: Given, 2C8H18(l) + 25 O2(g) --> 16CO2(g) + 18H2O(l) Excess reactant - O2 gas molar mass of…

Q: For the following reaction, 3.66 grams of oxygen gas are mixed with excess propane (C3Hg). The…

A: Given, 3.66 g oxygen gas are mixed with excess propane (C3H8). The chemical reaction, C3H8(g) +…

Q: If you are given 2.50 g C2H4 and 2.75 g of O2 to conduct the combustion reaction written below: C2H4…

Q: Gypsum casou2Hq 3. Propane is used as a fuel, commonly in portable grills. If 15.0 grams of propane…

Q: Acid rain results from the reaction of nitrogen dioxide, a major component of photochemical smog…

Q: What is the minimum mass of oxygen required to react completely with 4.90 g of C7H6O3? The…

Q: The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O:…

Q: What is the maximum yield of water (MW = 18.0 g/mol) when 2.80 moles of N2H4 gas are reacted with…

A: step-1 N2H4(g) +7 O2 (g) →2 N2O5 (g) +4 H2O (g) 2.80 moles 11.7 moles

Q: How many moles of water are produced when 6.33 moles of CH4 react? CH4 (g) + 2O2 (g) --> CO2 (g) +…

Q: Airbags are present in all new cars being produced today. When a collision occurs, a sensor sends an…

Q: Calculate the mass of H2O formed by burning 4.00 g of C2H5OH. The reaction is C2H5OH (l) + 3O2 (g)…

Q: Under appropriate reaction conditions Ag and S produce Ag2S according to the equation 2Ag + S → Ag2s…

A: Balanced reaction: 2Ag + S ....> Ag2S Mass of Ag = 28.6 g Molar mass of Ag = 107.9g/mol Moles of…

Q: In respiration process, one molecule of C6 H12O6 reacts with oxygen and produces water and CO2. Now,…

A: In the respiration mechanism, the oxygen is treated with the molecule C6H12O6 to generate the…

Q: Molar mass pf Ca (IO3)2 =40+2 (126+3 (16)) =40+2(126+48) =40+2 (174) = 40+348 =388g/mol Mass of…

A: Given Actual Yield = 6.72 gram Theoretical Yield = 7.275 gram Percentage Yield =…

Q: Part 2: Non-Mass-Ma 5. Ammonia is made by reacting nitrogen and hydrogen according to the following…

A: ****please note as you didn't ask for particular que number in solving first question for you**…

Q: Determine the theoretical yield of H2S (in moles) if 4.0 mol Al2S3 and 4.0 mol H2O are reacted…

A: In order to solve this question, we will be using simple mole concepts and the reaction provided…

Q: Acrylonitrile (C3H3N) is the starting material for many synthetic carpets and fabrics. It is…

A: The number of moles for a given compound or a molecule refers to the ratio of its mass to the…

Q: During studies of the reaction ,2N₂H₄(l)+N₂O₄(l)→3N₂(g) +4H₂O(g) a chemical engineer measured a…

A: Mass of each reactant used = 100 grams each Mass of NO formed = 10.0 grams Determination of mass of…

Q: Each step in the following process has a yield of 60.0%. CH₂ +4Cl₂ ⇒ CCI₂ + 4HCI CCI + 2 HF →→…

Q: When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water and oxygen…

Q: Ethanol (C2H5OH) is synthesized for industrial use by the following reaction, carried out at very…

Q: According to the reaction below you are supposed to produce 1 mol of SigN4 ,Silicon Nitride each…

A: Given, The reaction: 3Si(s) + 2N2(g) ---------> Si3N4(g) The produced moles of Si3N4 =0.743…

Q: Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen…

A: A numerical problem based on mole concept. Using the molecular mass of the reactants and products…

Q: Tungsten Carbide (WC), used in making tools and jewelries, is produced by the reaction of tungsten…

A: Given: Practical yield of WC = 10.8 g Let theoretical yield of WC = y g By stoichiometry of…

Q: how many grams of O2 are formed when 55.0g of KNO3 decomposes according to the following balanced…

A: 4KNO3(s) →2K2O(s) + 2N2(g) + 5O2(g) Reactants: KNO3 Products: K2O, N2 and O2

Q: 2. Explosives are effective if they produce a large number of gaseous molecules as products.…

Q: 5. The energy in our bodies mainly comes from carbohydrates, which are broken down into simple…

Q: According to the balanced reaction below, calculate the moles of NO2 that form when 5.20 x 10-3 mol…

Q: Liquid octane (CH3(CH2)6CH3) reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2…

Q: For the reaction represented by the equation CH4+2O22-->2H2O+CO2 calculate the percentage yield of…

A: Percentage yield of carbon dioxide

Q: Consider the reaction of NO and CO to form N2 and C02, according to the balanced equation: 2 NO (g)…

Q: Given the following balanced equation: 2 KHCO3 (s) --> K2CO3 (s) + H2CO3 (g) Molar mass of…

A: According to the law of conservation of mass, "Total mass of the reactant is equaled to the total…

Q: Propane combusts via the following unbalanced reaction: C3H8+O2→H2O+CO2 When 36.15 g of propane is…

Q: Consider the following combustion reaction: 2 C6H14 + 19 O₂ → 12 CO₂ + 14 H₂O How many moles of O₂…

Q: Liquid hexane CH3CH24CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide…

Question

19. When 0.75 moles chromium(III) oxide reacts with 2.5 moles hydrogen sulfide (H2S)
gas, chromium(III) sulfide and water were formed. What is the percent yield of Cr2S3 if
125 grams of it was obtained?
MW: Cr2S3 = 200.19g/mol
Cr2O3(s) + 3H2S(g) -> Cr2S3(s) + 3H2O()

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 with 3 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

18. Ammonium bicarbonate, which was classically obtained from deer antlers, is still used for baking in some European countries. It may be formed according to the following equation: NH3(aq) + CO2(aq) +H2O(1)→ NH4HCO3(aq) If 70.83g NH3, 110.12g CO2 and 3.12moles of H2O are reacted how many grams of NH4HCO3 can at most be made?
2NO(g) + O2(g) → 2NO2(g) You are provided with 4.12 molmol of nitrogen monoxide gas. Using the balanced chemical equation completed in Part A, determine how many moles of oxygen gas are needed to completely react with the nitrogen monoxide gas and how many moles of nitrogen dioxide are formed as a result? Ammonia and oxygen react to form nitrogen monoxide and water. Construct your own balanced equation to determine the amount of NO and H2O that would form when 2.80 molmol NH3 and 4.64 mol O2 react. Express the amounts in moles to two decimal places separated by a comma.
6.0L of O2 react with excess Sulfur dioxide gas. All gases are kept at the same temperature, pressure, and volume. What will be the theoretical yield of Sulfur trioxide gas in Liters? 2SO2(g) + O2(g) ----> 2SO3(g)
6. Hydrogen and iodine react to produce hydrogen iodide. If 3 moles hydrogen and 3 moles iodine react to produce 163 grams of hydrogen iodide, what is the percent yield? Assume constant temperature and pressure. The molar mass of H2 is 2.02 g/mol, of 12 is 253.8 g/mol, and of HI is 127.9 g/mol. H2(g) +12(g) → 2 HI(g)
In a certain ecperiment, 50 g of sodium chloride is reacted with 75.0 g of sulfuric acid, and 52.0g of sodium sulfate is produced. Determine the percent yield for this reaction. Unbalanced equation: NaCl (s) +H2SO4(i) -> HCl(g) + Na2SO4(s)
To produce zinc metal, carbon monoxide reacts with zinc (I1) oxide according to: Zno + CO - Zn + CO2 The carbon monoxide, however, is initially prepared from: 2C+ 02 → 200 How many grams of zinc metal (Zn) may be prepared if If 81.0g of C is used with excess amount of ZnO? Your answer should be numerical and neglect units (e.g., if you calculate 3.5g then input 3.5).
Ca(OH)2 (s) + H₂S(g) →→→ CaS (s) + 2H₂O(l) In the reaction above, calcium hydroxide and hydrogen sulfide react to form calcium sulfide and water. If you combine 11 g of hydrogen sulfide with 15 g of calcium hydroxide: 1) Which reactant is limiting? [Select] 2) Calculate the number of moles of calcium sulfide produced if the percent yield is 100%. [Select] ✓ mol Cas
Find the Mass to Mass Stoichiometry Calculutation using this formula: CaS5 + HCl → S + CaCl2 + H2S whereas here are the other given: Raw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g precipitated sulfur
Each step in the following process has a yield of 60.0%. CCl₂ + 4HCI → CCL₂F₂ + 2HCl The CCI, formed in the first step is used as a reactant in the second step. If 5.00 mol CH₂ reacts, what is the total amount of HCI produced? Assume that Cl₂ and HF are present in excess. CH4 + 4Cl₂ CCl₂ + 2 HF moles HCl: 12.48 Incorrect mol
K $ 4 R For the following reaction, 4.16 grams of hydrogen gas are allowed to react with 45.2 grams of iodine hydrogen (g) + iodine (s)→ hydrogen iodide (g) What is the maximum amount of hydrogen iodide that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? Submit Answer % 5 [Review Topics] [References] Use the References to access important values if needed for this question. Show Hint T Retry Entire Group 4 more group attempts remaining Cengage Learning Cengage Technical Support < 6 Y d 7 U 8 I < ( 9 0 O P grams grams * Previous 4) [
#10pls
Liquid octane (CH3(CH2)6CH3) reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. If 64.0g of water is produced from the reaction of 92.52g of octane and 181.4g of oxygen gas, calculate the percent yield of water.