Consider the balanced chemical reaction below. What is the maximum amount of grams of Fe that can be produced from 33.4 g iron(III) oxide mixed with 47.2 g carbon monoxide?
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- You have a chemical in a sealed glass container filled with air. The setup is sitting on a balance as shown below. The chemical is ignited by means of a magnifying glass focusing sunlight on the reactant. After the chemical has completely burned, which of the following is true? Explain your answer. a. The balance will read less than 250.0 g. b. The balance will read 250.0 g. c. The balance will read greater than 250.0 g. d. Cannot be determined without knowing the identity of the chemical.When benzene (C6H6) reacts with bromine (Br)2, bromobenzene(C6H5Br) is obtained:C6H6 + Br2-------->C6H5Br + HBr(a) When 30.0 g of benzene reacts with 65.0 g of bromine, whatis the theoretical yield of bromobenzene? (b) If the actual yieldof bromobenzene is 42.3 g, what is the percentage yield?3. In a blast furnace, iron (III) oxide reacts with coke (carbon) to produce molten iron and carbon monoxide:Fe2O3 + 3C --> 2 Fe + 3 COHow many kilograms of iron would be formed from 125 kg of Fe2O3?
- N2(g)+3H2(g)--->2NH3(g) If 20.0 moles of ammonia (N H 3) are needed for a particular process, how many moles of diatomic Nitrogen (N 2) are needed?13. If kerosene is represented by the formula C14H30 and has a density of 0.763 g/mL, how many grams of CO2 are produced by the combustion of 7.53 L of kerosene in an indoor heater?Aniline (C6H5NH2) can be produced from chlorobenzene (C6H5Cl) via the following reaction: C6H5Cl (l) + 2 NH3 (g) ⟶ C6H5NH2 (l) + NH4Cl (s) Assume that 20.0 g of chlorobenzene at 92% purity is mixed with 8.30 g of ammonia. a) Which is the limiting reactant? b) Which reactant is present in excess? c) What is the theoretical yield of ammonium chloride in grams? d) If 4.78 g of NH4Cl was recovered, what was the percent yield? e) How many grams of a the limiting reagent must be used to isolate 10.20 g of C6H5NH2? Assume this is a separate experiment than the one described above. Also assume a purity of 92% for chlorobenzene and the same percent yield.
- Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: 5Ca + V2O5 --->5CaO + 2V In one process, 1.540×103 g of V2O5 react with 2.100×103 g Ca. (a) Calculate the theoretical yield of V. _________ g (b) Calculate the percent yield if 807.0 g of V are obtained. __________ % Report your answers to the correct number of significant figures.Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: 5Ca + V2O5 longrightarrow 5CaO + 2V In one process, 1.540 × 103 g of V2O5 react with 2.120 × 103 g Ca. (a) Calculate the theoretical yield of V. g (b) Calculate the percent yield if 807.0 g of V are obtained. % Report your answers to the correct number of significant figures.Consider the following reaction: Zn(s) + MoO3(s) --> Mo2O3(s) + ZnO(s) a. 80.0 grams of molybdenum (VI) oxide reacts with 17.0 grams of zinc. Determine the limiting reactant b. If, in the above situation, only 0.260 moles of zinc oxide, ZnO was produced. i. What mass of zinc oxide was produce? ii. What was the percentage yield of the reaction? PLEASE SHOW WORK FOR ALL QUESTIONS!!!
- 4 Fe + 3 O2 ⟶⟶ Fe2O3 If you run a reaction with the balanced equation from above that has a theoretical yield of 245 g, how many grams of Fe were reacted initially if the it was run with an excess of O2? (Hint-This is just a stoichiometry problem working in the opposite direction.) Group of answer choices A. 85.7 g Fe B. 42.8 g Fe C. 171 g Fe D. 3.07 g FeCephalexin is a semisynthetic cephalosporin antibacterial drug intended for oral administration. Cephalexin is an organic compound that has a molecular formula of C16H17N3O4S. If a medication bottle containing a suspension of cephalexin reads 0.720 g/0.5 cL, how many moles of cephalexin were administered to a patient which was given a dose of 12 mL?Imagine that you are working on ways to improve the process by which iron ore containing Fe2O3 is converted into iron. In your tests you carry out the following reaction on a small scale: Fe2O3 (s) + CO (g) ---> Fe (s) + CO2 (g)(a) If you start with 150 g of Fe2O3 as the limiting reagent, what is the theoretical yield of Fe? (b) If the actual yield of Fe in your test was 87.9 g, what was the percent yield?