27) SEP Apply Mathematical Concepts When 84.8 g of iron(III) oxide react with an excess of carbon monoxide, iron is produced. What is the theoretical yield of iron? Fe,O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)
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- 75.4 grams of C2H3Br3 reacts with 47.1 grams of O2 to produce CO2. 4C2H3Br3 + 11O2 → 8CO2 + 6H2O + 6Br2 Actual yield 47. g,Find Percent yield and theoretical yieldPRACTICE ANOTHER C4H10 + O2 → CO2 + H2O (unbalanced)What mass of CO2 is produced in the complete combustion of 78.8 g of butane, C4H10, to CO2 and H2O? gWhat mass of oxygen is required for the complete reaction? gWhat mass of water is produced? gIn the acetylene torch, acetylene gas (C2H2) burns in oxygen to produce carbon dioxide and water. 2C2H2 (g) + 5O2(g) à 4CO2(g) + 2H2O (g) Find the moles of CO2produced when 2.5 moles C2H2are burnt? Your Answer: Question 16 options: Answer units
- A chemistry student performed the reaction: SnCl4(l) + 2H2Se(g) -> SnSe2(s) + 4HCl(g) in lab. The student started with 0.34 moles of SnCl4 and 0.46 moles of H2Se. The amount of HCl(g) actually produced by the student was 0.26 moles of HCl. a. what is the limiting reagent? b. what is the % yield for this reaction?Based on the graph below calculate the ratio of moles of H2O to moles of anhydrous KAl(SO4)2. Show all work including units. Note: Report the ratio to the closest whole number. Aluminum Cup (Empty) 2.50 Aluminum Cup + 2.0 grams of Alum 4.50 Aluminum Cup + Alum After 1st Heating 3.60 Aluminum Cup + Alum After 2nd Heating 3.60 Mass of Released H2O 1.10 Molar mass of H2O 18.016 Moles of Released H2Oe) If only 0.105 grams of hydrogen gas actually form, what is the percent yield for this reaction? [ Select ] ["1.9 %", "3.55 %", "28.1 %", "114 %"]
- In the following reaction, oxygen is the excess reactant.SiCl4 + O2 → SiO2 + Cl2The table shows an experimental record for the above reaction. Experimental Record Trial Starting Amount of SiCl4 Starting Amount of O2 Actual Yield of SiO2 1 150 g 200 g 49.2 g 2 75 g 50 g 25.2 g Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work. Based on the percentage yield in Trial 2, explain what ratio of reactants is more efficient for the given reaction. Source StylesNormalIn the following reaction, oxygen is the excess reactant.SiCl4 + O2 → SiO2 + Cl2The table shows an experimental record for the above reaction. Experimental Record Trial Starting Amount of SiCl4 Starting Amount of O2 Actual Yield of SiO2 1 120 g 240 g 38.2 g 2 75 g 50 g 25.2 g Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work. Based on the percentage yield in Trial 2, explain what ratio of reactants is more efficient for the given reaction.Stoichiometry answer all please 1. Balance this equation:C 2 H 5 OH (l) + O 2(g) CO 2(g) + H 2 O (g)a. Interpret the equation in terms of numbers of molecules and moles.b. Show that the balanced equation obeys the law of conservation of mass. 2. Isopropyl alcohol (C 3 H 7 OH) burns in air according to this equation:C 3 H 7 OH (l) + O 2(g) CO 2(g) + H 2 O (g)a. Calculate the moles of oxygen needed to react with 3.40 mol C 3 H 7 OH.b. Find the moles of each product formed when 3.40 mol C 3 H 7 OH reacts with oxygen. 3. Hydrofluoric acid cannot be stored in glass bottles because compounds called silicatesin the glass are attacked by the HF. Sodium silicate reacts as follows:Na 2 SiO 3(s) + HF (aq) H 2 SiF 6 (aq) + NaF (aq) + H 2 O (l)a. How many moles of HF are needed to react with 0.300 mol of Na 2 SiO 3 ?b. How many grams of NaF form when 0.500 mol of HF reacts with excess Na 2 SiO 3 ?c. How many grams of Na 2 SiO 3 can react with 0.800 g of HF?
- A chemist wants to extract copper metal from copper chloride solution. The chemist places 0.25 grams of aluminum foil in a solution of 0.40 grams of copper (II) chloride. A single replacement reaction takes place. What are the likely observations when the reaction stops?Unbalanced equation: CuCl2 + Al → AlCl3 + Cu About 0.90 grams of copper is formed, and some aluminum is left in the reaction mixture. About 0.20 grams of copper is formed, and some aluminum is left in the reaction mixture. About 0.90 grams of copper is formed, and some copper chloride is left in the reaction mixture. About 0.20 grams of copper is formed, and some copper chloride is left in the reaction mixture.Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in moles CO₂ from the complete combustion of 29.3 grams CH₄ according to the following balanced chemical equation: 1 CH₄(g) + 2 O₂(g) → 1 CO₂(g) + 2 H₂O(l)observe the following balanced chemical equation: 6 NH3(g) + 8 O3(g) --> 3 N2O5(g) + 9 H2O(g) if the reaction of 2.0 mol NH3(g) and 2.5 mol of O3(g) is run with 100% efficiency which of the followng is correct? all NH3(g) will be consumed 60.0 g of water will be produced all of the O3(g) will be consumed 1.0 mole of N2O5(g) will be produced