QUESTION 17 The reaction of 25.0 g benzene, C6H6, with excess HNO3 resulted in 21.4 g C6H5NO2. What is the percentage yield? C6H6 + HNO3 → CGH5NO2 + H2O O 100 % O 27.4 % O 54.3% O 85.6 % QUESTION 18 P Type here to search %3 林 5:41 PM E 4) * ENG 5/6/2021 hyp
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- Answer the following: A 0.498g sample contains 26.0% aluminum triiodide, All3, (MW=407.695) by weight. What is the mass of aluminum triiodide in the sample? If the sample is reacted with silver nitrate, AgNO3, to precipitate silver iodide, Agl, what will be the stoichiometric ratio of AgNO3 to All3? What is the maximum mass of Agl (MW=234.77) that can be produced from the sample?Please answer #1 with part a-e. Show demensional analysis work please. 1. Combustion of hexane: 2C6H14 (g) + 19O2 (g) --> 12CO2 (g) + 14H2O (g) a. Balance the reaction by writing the correct coefficients in front of the reactants and products. b. If you started with 7.77 moles of hexane, how many moles of carbon dioxide could be produced? c. If you started with 8.11 grams of hexane, how many moles of carbon dioxdie could be produced? d. How many grams of oxygen gas are needed to react with 25.0 moles of hexane? e. What mass of water vapor, in kg, could be produced from combustion of 55.3 kg of hexane?Refer to the reaction below in which two compounds, Hydrazine and Dinitrogen tetroxide combine to yield nitrogen gas and water. 2 N2H4(g) + N2O4(g) + 3N2(g) + 4 H2O(g) a. When 0.25 moles of N2H4 reacts with excess N2O4 what is the mass of H2O that is produced? Video: b. If the actual mass of water formed is 6.30 grams what is the percent yield?
- A complete combustion of octane, C8H18, a component of gasoline, proceeds as: C8H18(l ) + O2(g) → CO2(g) + H2O(l) {unbalanced equation} Atomic weights (g/mol): C=12, H=1, O=16 500 grams of oxygen is made to react with an excess amount of octane. What is the percent yield if 312 grams of carbon dioxide is actually produced? Enter final answer with TWO decimal places (e.g. 37.18 or 35.00 or 98.20); numeric answers only, do not include the units.Please answer c and D A student conducts this synthesis. She starts with 7.3447 g of Fe(NH4)2(SO4)2 6H2O and isolates 4.8251 g of K3[Fe(C2O4)3] 2H2O product. a. Assuming all Fe(NH4)2(SO4)2 6H2O reacts, how many moles of FeC2O4 should form in the first reaction? Answer: 0.019 moles b. How many moles of FeC2O4 should form in the first reaction? Answer: 0.019 moles c. How many grams of K3[Fe(C2O4)3] 2H2O should form (This is the theoretical yield)? Group of answer choices A)1.25 grams B)9.20 grams C)8.30 grams D)4.25 grams D. What is the student’s actual yield (mass) and percent yield of K3[Fe(C2O4)3] 3H2O? Group of answer choices A)25.45 % B)52.45 % C)10.5 % D)100%Balanced equation: C7H802+ 9O2= 7CO2+4H2O If you reacted 12.0 g of C7H8O2 with200.0 g of O2, what mass (in g) ofH2O can you theoretically make? _________________________ g b.For problem 2a (above), write the formula of the limiting reagent?______________________________ c.For problem 2a (above), write the formula of the excess reagent?d.If your actual yield was 3.50 g of H2O, what is your percent yield?___________________________ %
- Hydrofluoric acid (HF) can be prepared according to the reaction: CaF2 + H2SO4 à 2 HF + CaSO4. In one experiment, 42.0 g of CaF2 was treated with excess H2SO4 and a yield of 14.2 g of HF was obtained. What is the theoretical yield of HF? (show work please)A compound containing carbon, hydrogen, and oxygen contains 60.00% carbon by mass and8.05% hydrogen by mass.d) If 10.0 grams of this compound is burned in 10.0 grams of oxygen:i) What is the limiting reagent, or is the mixture stoichiometric?ii) What is the theoretical yield of water vapor?iii) If the actual yield is 2.42 g of water vapor, what is the % yield for the reaction? (a-c already answered/completed)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 Fe
- 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 yieldWhat is the minimum mass of oxygen required to react completely with 4.90 g of C7H6O3? The unbalanced chemical equation is shown below. Choose the closest value. (pick one option) C7H6O3C7H6O3(s) + O2O2(g) ⟶⟶ CO2CO2(g) + H2OH2O(g) Molar masses (in g mol−1−1) 138.12 32.00 44.01 18.02 1. 7.95 g of O2O2 are required 2. 148 g of O2O2 are required 3. 21.1 g of O2O2 are required 4. 1.14 g of O2O2 are required 5. 4.54 g of O2O2 are requiredPlease write out all the formulas and steps: Known: 5 % NaOCI: Molar mass of = 165.15 g/mol Quantity in mL= 319.99 mL Density in g/mL= 1.11 g/mL Find moles= ??? 10% NaOH: Molar mass of = 39.997 g/mol Quantity in mL= 20 mL Density in g/mL= 1.11 g/mL Find moles= ??? m-nitrobenzoic acid: Molar mass= 167.12 g/mol Grams obtained= 7.435g Theoretical yield= ???g Percent yield= ??? %