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 ?

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?

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