Aluminum trichloride, AlCl3AlCl3, is formed from the reaction of Al2O3(s)Al2O3(s) with HClHCl gas. The balanced reaction is Al2O3(s)+6HCl(g)→2AlCl3(s)+3H2O(g)Al2O3(s)+6HCl(g)→2AlCl3(s)+3H2O(g) When 1.70 kgkg of Al2O3Al2O3 is reacted with excess HClHCl until it is all consumed, 3.25 kgkg of AlCl3AlCl3 are recovered after the reaction is completed. What is the percent yield for this experiment?

Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite, involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide: 2 MNCO;(s)+O,(g)→2 MnO,(s)+2 CO,(9) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide: 3 MnO2(s)+4 Al(s)→3 Mn(s)+2 Al,O3(s) Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced.

Consider the reaction.   2Al(s)+Fe2O3(s)−→−heatAl2O3(s)+2Fe(l)2Al(s)+Fe2⁢O3⁡(s)→heatAl2⁢O3⁡(s)+2Fe(l)   If 18.3 kg Al18.3 kg Al reacts with an excess of Fe2O3,Fe2⁢O3, how many kilograms of Al2O3Al2⁢O3 will be produced? mass of Al2O3Al2⁢O3 produced:

You carefully weigh out 11.00 g of CaCO3 powder and add it to 44.55 g of HCl solution. You notice bubbles as a reaction takes place. You then weigh the resulting solution and find that it has a mass of 51.04 g . The relevant equation is CaCO3(s)+2HCl(aq)→H2O(l)+CO2(g)+CaCl2(aq) Assuming no other reactions take place, what mass of CO2 was produced in this reaction?

Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite, involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide: 2 MnCO3(s) + O₂(g) 2 MnO₂ (s) +2 CO₂(g) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide: 3 MnO₂ (s) +4 Al(s)-3 Mn(s)+2 Al₂O3(s) Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced. 0 Continue * FOR 80 FS F4 F5 0-0 X MacBook Air F6 4 Ś F7 A DI FB © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center F9 A Submit A F10

One of the reactions in the Solvay Process involves the reaction of calcium oxide with water toproduce slaked lime (calcium hydroxide).CaO(s) + H O2 (l) - Ca(OH)2 (s)A lab technician performs the experiment and uses 54.8 g of calcium oxide to react with a setamount of water. When the reaction is completed, the technician uses a filtration apparatus tocollect the mass of calcium hydroxide produced.    The following data is recorded:Mass of filter paper: 1.24 gMass of filter paper and solid: 68.04 g What is the theoretical mass of calcium hydroxide that is predicted to be produced? What mass of precipitate was collected in this experiment? What is the percent error? Comment on the validity of the results

CH3OH(l) + CO(g)                    HC2H3O2(l)      In an experiment, 15.0 g of methanol and 10.0 g of carbon monoxide were placed in a reaction vessel. What is the          theoretical yield of acetic acid? If the actual yield is 19.1 g, what is the percentage yield?

In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation: Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g) The molar masses for each compound in the equation are as follows;  PCl5: 208.224 g/mol H2O: 18.015 g/mol H3PO4: 97.994 g/mol HCl; 36.45 g/mol   Based on the information above and the information attached explain in WORDS why PCl5 is the limiting reagent.

Silicon carbide or carborundum is a widely used ceramic material in car brakes and bullet-proof vests because of its hardness. Carborundum is found naturally in the mineral moissanite, but the demand for it exceeds the supply. For this reason it is generally synthesized in the laboratory. The reaction is: SiO2 + 3 C→SiC + 2 CO How many kg of silicon carbide can be formed by the reaction of 250.0 kg of sand (SiO2) with excess carbon?

Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3C4H6O3) with salicylic acid (C7H6O3C7H6O3) to form aspirin (C9H8O4C9H8O4) and acetic acid (C2H4O2C2H4O2). The balanced equation isC4H6O3+C7H6O3→C9H8O4+C2H4O2C4H6O3+C7H6O3→C9H8O4+C2H4O2In a laboratory synthesis, a student begins with 3.10 mLmL of acetic anhydride (density=1.08gml−1density=1.08gml−1) and 1.23 gg of salicylic acid. Once the reaction is complete, the student collects 1.22 gg of aspirin.    Determine the percent yield of aspirin for the reaction. Express your answer using three significant figures.