Alternative method The company is developing a "greener" method of making propene oxide from propene using hydrogen peroxide, H₂O2, in supercritical water with a vanadium catalyst. In the reaction 1.00 kg of vanadium catalyst and 32.0 kg of water are used for each kilogram of propene. 75% of the vanadium catalyst can be collected and reused in a subsequent batch: V, H₂O C3H6+ H2O2C3H6O + H₂O Consider the prices of the following substances. 89.0% yield Part B There is virtually no waste produced with this green process and there is no waste disposal fee, but the yield is only 89.0%. $ Substance LGI ΑΣΦΑ propene hydrogen peroxide vanadium catalyst supercritical water propene oxide Calculate the profit from producing 75.00 kg of propene oxide by this alternative green process. Express your answer numerically in dollars using three significant figures. ► View Available Hint(s) Submit Price per unit Unit $10.97 kg $1.96 kg $57.50 kg $1.85 kg $258.25 kg ?

Alternative method The company is developing a "greener" method of making propene oxide from propene using hydrogen peroxide, H₂O2, in supercritical water with a vanadium catalyst. In the reaction 1.00 kg of vanadium catalyst and 32.0 kg of water are used for each kilogram of propene. 75% of the vanadium catalyst can be collected and reused in a subsequent batch: V, H₂O C3H6+ H2O2C3H6O + H₂O Consider the prices of the following substances. 89.0% yield Part B There is virtually no waste produced with this green process and there is no waste disposal fee, but the yield is only 89.0%. $ Substance LGI ΑΣΦΑ propene hydrogen peroxide vanadium catalyst supercritical water propene oxide Calculate the profit from producing 75.00 kg of propene oxide by this alternative green process. Express your answer numerically in dollars using three significant figures. ► View Available Hint(s) Submit Price per unit Unit $10.97 kg $1.96 kg $57.50 kg $1.85 kg $258.25 kg ?

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...

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The reaction for the oxidation of NH3 is given as: 4 NH3 + 5 024 NO + 6H₂O Under certain conditions the reaction will proceed at 29.8% yield of NO. How many grams of NH3 must be used to react with excess oxygen to yield 70.5 g of NO? Hint: 70.5 g of NO is the actual yield. 21.0 134 237 2.37 None of these responses apply.
4 dicmal point
If the yield of the reaction is 76.7%, what is the actual yield of chlorine?
Ammonia (NH3) is naturally produced through the decomposition of organic material as wellas being high in wastewater discharged to natural waters. In the environment it is oxidizedto form nitrite (NO2-), and nitrite is then oxidized to form nitrate (NO3-) in a process callednitrification. The balanced equations are given below:2NH3 + 3O2 → 2NO2- + 2H+ + 2H202NO2- + O2 → 2NO3-a) Assuming complete oxidation, what is the theoretical oxygen demand to convert100mg/L of ammonia to nitrate (i.e., how much oxygen is necessary)? Report youranswer as mg/L of O2.Answer: 376 mg/L O2b) This conversion process makes water more acidic. With reference to the equations forpH, explain why this occurs
The extraction of aluminum metal from the aluminum hydroxide in bauxite ore by the Hall-Héroult process is one of the most remarkable success stories of late 19th century practical chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina and water: 2 Al(OH)3(s)-Al₂O3(s) + 3 H₂O(g) In the second step, alumina and carbon react to form aluminum and carbon dioxide: 2 Al₂O3(s)+3 C(s)-4 Al(s) + 3 CO₂(g) Write the net chemical equation for the production of aluminum from aluminum hydroxide and carbon. Be sure your equation is balanced. Explanation Check 80 E5 ローロ X On F6 S MacBook Air F7 DII FB FO A Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Access F10 A F11 ola Ar 00
1. Chlorine has two isotopes, 35Cl and 37Cl. Which isotope has a higher natural abundance? Show your calculations. U 2. Extraction of aluminum from Bauxite ore starts with the following reaction: a Al₂O3 + b NaOH → c NaAlO₂ + d H₂O (a) Balance the equation, i.e., specify the values of a. b. c, and d. (b) Assuming a theoretical reaction yield, at what mass will Al₂O3 no longer be a limiting reagent in a process that also uses 40 ko of sodium hydroxide?
Antimony is produced by heating powdered antimony trisulphide with iron and removing the molten antimony from the reaction vessel. If 1.8 kg of antimony trisulphide and 1.3 kg of iron are heated to give 0.9 kg of antimony. The reaction is as follows: Sb2S3 + 3Fe --> 2Sb + 3FeS The amount of percentage excess of the Excess Reactant is: The amount of percentage excess of the Excess Reactant is: 46.45% 52.77% 47.53% 69.75% The degree of completion of the reaction is: 46.45% 52.77% 47.53% 69.75% The percentage conversion of iron is: 46.45% 52.77% 47.53% 69.75%
Balance the following equations, name reactants and products, name reactions type and prove oxidation/reductions K2SO4 + BaCl2 —> BaSO4 + KCL
1) Balance all these equations. (Hint, only small numbers are nceded) 2) Determine the theoretical yield of the final solid if you use 20.000g NaHCO3 Possible equations for the decomposition. Mass of just the NaHCO Theoretical yicld of final solid A NAHCO3 () > NazCO3 H20 (6) CO2 - - _NaHCO, (a) → NazCO () +_H20 +_CO2 B - C - NAHCO3 ) > CO2 NaOH (0) - NaHCO3 (4) -> Na20 (0) + H20 +. -
In a closed system, equal amounts of ammonia and oxygen react to produce nitrogen monoxide and water. What is the limiting reactant? NH3 4NH3 + 502 - 4NO + 6H,0 NO H20 OO O
Atomic Weight of a Metal from Hydrogen Gas Production Objective: To produce hydrogen gas by reaction of a metal with an acid. To use the ideal gas equation to determine the atomic weight of the metal. Background: Many metals react with hydrochloric acid to produce hydrogen gas and metal ions. In this Lab you will use Magnesium: Mg(s) + 2 H+(aq) → H2(g) + Mg2+(aq) The moles of hydrogen gas produced can be determined using the Ideal Gas equation, PV = nRT. From the moles of hydrogen and the stoichiometry (reacting ratios) of the reaction, it will be possible to calculate how many moles of metal reacted. From this, the atomic weight of the metal will be determined. When a gas is collected over water, it becomes saturated with water vapor and the total pressure of the mixture in the buret equals the partial pressure of the gas plus the partial pressure of the water vapor. The partial pressure of water vapor depend on temperature. Finally, the total pressure of gas…
Write a balanced chemical equation for the formation of 1 mol of Cr₂O3(s) from Cr and O2 in their standard states. (Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit.) ✓+3/20₂(g) ✓- →Cr₂O3(s) 2Cr(s) The equation of the formation of Cr₂O3 (s) from the elements: 2 Cr(s) + 3/2 O2(g) → Cr₂O3(s) b What is the enthalpy change if 3.1 g of chromium is oxidized to Cr₂O3(s)? AfH for Cr₂O3 (s) is -1134.7 kJ/mol Enthalpy change = Submit Submit Answer OCT 30 kJ Try Another Version tv ♫ 10 item attempts remaining 5 LIZA O Cengage Learning Cengage Technical Support Correct 144 B MacBook Pro * 23 Ⓡ E Previous Next Email Instructor Save and Exit U