23:19How to Calculate Percent Yield and Theoretical Yield The Best Way - TUTOR HOTLINEMelissa Maribel402
Open QuestionAmmonia, NH3, reacts with hypochlorite ion, OCl–, to produce hydrazine, N2H4. How many grams of hydrazine are produced from 115.0 g NH3 if the reaction has a 81.5% yield? 2 NH3 + OCl– → N2H4 + Cl– + H2O171553Has a video solution.
Multiple ChoiceThe reduction of iron (III) oxide creates the following reaction: Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H2O (g) If the above reaction only went to 75% completion, how many moles of Fe2O3 were require to produce 0.850 moles of Fe? 91213Has a video solution.
Multiple ChoiceGold metal can be reduced from the compound gold sulfide by hydrogen gas according to the following balanced chemical equation: Au2S3 + 3 H2 → 3 H2S + 2 Au How many grams of Au can be produced from 500.20 g of Au2S3 and 5.67 g H2?77
Multiple ChoiceCyanogen (CN)2 has been observed in the atmosphere of Titan, Saturn’s largest moon, and in the gases of interstellar nebulas. On Earth, it is used as a welding gas and a fumigant. In its reaction with fluorine, carbon tetrafluoride (CF4) and nitrogen trifluoride (NF3) gases are produced: (CN)2 + 7 F2 → 2 CF4 + 2 NF3 What is the percent yield of the reaction if 45.0 g of CF4 are isolated from the reaction between 75.0 g each of (CN)2 and F2?79
Multiple ChoiceWhat is the percent yield for a reaction in which 22.1 g Cu is isolated by reacting 45.5 g Zn with 70.1 g CuSO4? Zn (s) + CuSO4 (aq) → Cu (s) + ZnSO4 (aq)6133Has a video solution.
Textbook QuestionIf 42.85 grams of salicylic acid reacts with excess acetic anhydride and produces 48.47 grams of aspirin, what is the percent yield of the reaction? (LO 3.6) (a) 88.40% (b) 64.69% (c) 86.72% (d) 78.74%331Has a video solution.
Textbook QuestionNitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. (c) If the actual yield of the reaction was 75% instead of 100%, how many molecules of each kind would be present after the reaction was over? 447Has a video solution.
Textbook QuestionSilver sulfide, the tarnish on silverware, comes from the reaction of silver metal with hydrogen sulfide (H2S).The unbalanced equation is: Ag + H2S + O2 --> Ag2S + H2O Unbalanced If the reaction was used intentionally to prepare Ag2S, how many grams would be formed from 496 g of Ag, 80.0 g of H2S, and excess O2 if the reaction takes place in 90% yield? (LO 3.9) (a) 525 g (b) 1139 g (c) 583 g (d) 10251029Has a video solution.
Textbook QuestionMagnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2 Mg(s) + O2( g)¡2 MgO(s) When 10.1 g of Mg reacts with 10.5 g O2, 11.9 g MgO is collected. Determine the limiting reactant. Determine the theoretical yield. Determine the percent yield for the reaction.6770Has a video solution.
Textbook QuestionUrea (CH4N2O) is a common fertilizer that is synthesized by the reaction of ammonia (NH3) with carbon dioxide: 2 NH3(aq) + CO2(aq)¡CH4N2O(aq) + H2O(l ) In an industrial synthesis of urea, a chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 kg of urea. Determine the limiting reactant. Determine the theoretical yield of urea. Determine the percent yield for the reaction.5435Has a video solution.
Textbook QuestionMany computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.8 kg of SiO2 reacts with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine the percent yield for the reaction.983Has a video solution.
Textbook QuestionNickel(II) sulfate, used for nickel plating, is prepared by treat-ment of nickel(II) carbonate with sulfuric acid: NiCO3 + H2SO4 --> NiSO4 + CO2 + H2O (b) How many grams of NiSO4 are obtained if the yield is 78.9%?498Has a video solution.
Textbook QuestionHydrazine, N2H4, once used as a rocket propellant, reacts with oxygen: N2H4 + O2 --> N2 + 2 H2O (b) How many grams of N2 are obtained if the yield is 85.5%?747Has a video solution.
Textbook Question(b) Why is the actual yield in a reaction almost always less than the theoretical yield?349Has a video solution.
Textbook Question(a) Define the terms theoretical yield, actual yield, and percent yield.372Has a video solution.
Textbook QuestionAcetic acid (CH3CO2H) reacts with isopentyl alcohol (C5H12O) to yield isopentyl acetate (C7H14O2), a fragrant substance with the odor of bananas. If the yield from the reaction of acetic acid with isopentyl alcohol is 45%, how many grams of isopentyl acetate are formed from 3.58 g of acetic acid and 4.75 g of isopentyl alcohol? The reaction is CH3CO2H + C5H12O ---> C7H14O2 + H2O968Has a video solution.
Textbook QuestionCisplatin [Pt(NH3)2Cl2], a compound used in cancer treat-ment, is prepared by reaction of ammonia with potassium tetrachloroplatinate: K2PtCl4 + 2 NH3 ----> 2 KCl + Pt(NH3)2Cl2 How many grams of cisplatin are formed from 55.8 g of K2PtCl4 and 35.6 g of NH3 if the reaction takes place in 95% yield based on the limiting reactant?848Has a video solution.
Textbook QuestionIf 1.87 g of acetic acid (CH3COOH) reacts with 2.31 g of isopentyl alcohol (C5H12O) to give 2.96 g of isopentyl acetate (C7H14O2), what is the percent yield of the reaction?401Has a video solution.
Textbook QuestionIf 3.42 g of K2PtCl4 and 1.61 g of NH3 give 2.08 g of cispla-tin (Problem 3.81), what is the percent yield of the reaction?278Has a video solution.
Textbook QuestionWhen benzene 1C6H62 reacts with bromine 1Br22, bromobenzene 1C6H5Br2 is obtained: C6H6 + Br2¡C6H5Br + HBr (b) If the actual yield of bromobenzene is 42.3 g, what is the percentage yield?4391Has a video solution.
Textbook QuestionWhen ethane 1C2H62 reacts with chlorine 1Cl22, the main product is C2H5Cl, but other products containing Cl, such as C2H4Cl2, are also obtained in small quantities. The formation of these other products reduces the yield of C2H5Cl. (a) Calculate the theoretical yield of C2H5Cl when 125 g of C2H6 reacts with 255 g of Cl2, assuming that C2H6 and Cl2 react only to form C2H2Cl and HCl. (b) Calculate the percent yield of C2H5Cl if the reaction produces 206 g of C2H5Cl.836Has a video solution.
Textbook QuestionHydrogen sulfide is an impurity in natural gas that must be removed. One common removal method is called the Claus process, which relies on the reaction: 8 H2S1g2 + 4 O21g2¡S81l2 + 8 H2O1g2 Under optimal conditions the Claus process gives 98% yield of S8 from H2S. If you started with 30.0 g of H2S and 50.0 g of O2, how many grams of S8 would be produced, assuming 98% yield?1171Has a video solution.
Textbook QuestionWhen hydrogen sulfide gas is bubbled into a solution of sodium hydroxide, the reaction forms sodium sulfide and water. How many grams of sodium sulfide are formed if 1.25 g of hydrogen sulfide is bubbled into a solution containing 2.00 g of sodium hydroxide, assuming that the sodium sulfide is made in 92.0% yield?1547Has a video solution.
Textbook QuestionAspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2). The balanced equation is: C4H6O3 + C7H6O3¡C9H8O4 + C2H4O2 In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g/mL) and 1.25 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin. Determine the limiting reactant. Determine the theoretical yield of aspirin. Determine the percent yield for the reaction.10273Has a video solution.
Textbook QuestionViridicatumtoxin B, C30H31NO10, is a natural antibiotic compound. It requires a synthesis of 12 steps in the laboratory. Assuming all steps have equivalent yields of 85%, which is the final percent yield of the total synthesis?177Has a video solution.
Textbook QuestionThe combustion of liquid ethanol (C2H5OH) produces carbon dioxide and water. After 4.62 mL of ethanol (density = 0.789 g>mL) is allowed to burn in the presence of 15.55 g of oxygen gas, 3.72 mL of water (density = 1.00 g>mL) is collected. Determine the percent yield for the reaction. (Hint: Write a balanced equation for the combustion of ethanol.)2183Has a video solution.
Textbook QuestionTitanium occurs in the magnetic mineral ilmenite (FeTiO3), which is often found mixed with sand. The ilmenite can be separated from the sand with magnets. The titanium can then be extracted from the ilmenite by the following set of reactions: FeTiO3(s) + 3 Cl2( g) + 3 C(s)¡3 CO(g) + FeCl2(s) + TiCl4( g) TiCl4( g) + 2 Mg(s)¡2 MgCl2(l ) + Ti(s) Suppose that an ilmenite–sand mixture contains 22.8% ilmenite by mass and that the first reaction is carried out with a 90.8% yield. If the second reaction is carried out with an 85.9% yield, what mass of titanium can be obtained from 1.00 kg of the ilmenite– sand mixture?1172Has a video solution.
