Percent Yield

Urea (CH4N2O) is a common fertilizer that is synthesized by the reaction of ammonia (NH3) with carbon dioxide: 2 NH3 (aq) + CO2 (aq)      →       CH 4N2O (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, theoretical yield of urea and percent yield for the reaction.  For the choices below, what is the percent yield? A. 70.0% B. 58.4% C. 84.9 % D. 79.2%

Hydrogen fluoride is used in the manufacture of Freon (which also destroys ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reaction CaF2 + H2SO4      →      CaSO 4 + 2HF  In one process, 6.00 kg of CaF 2 are treated with an excess of H 2SO4 and yield 2.86 kg of HF. Calculate the percent yield of HF. a) 76.3% b) 83.6% c) 89.2% d) 93.0% e) 97.8%

What is the percent yield for a reaction in which 28 g of Cu is produced by reacting 32.5 g of Zn in excess CuSO4 solution? Zn (s) + CuSO4 (aq) → Cu (s) + ZnSO4 (aq)   a. 88% b. 75% c. 60% d. 50%

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react with excess Al according to the following reaction. (Molar masses: Fe = 55.85 g/mol, O = 16.00 g/mol, Fe2O3 = 159.70 g/mol) Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)   A) 61.03 % B) 28.65 % C) 57.30 % D) 20.02 % E) 81.93 %

For the following balanced reaction, 4C6H5Cl + SiCl4 + 8Na → (C6H5)4Si + 8NaCl If the reaction produces (C6H5)4Si in a 96.3 % yield, then how many grams of C 6H5Cl will be necessary to make 152.0 g of (C6H5)4Si?    

One rather exotic compound synthesized by the Susan Latturner group is Ba 2In5P5. (See Chemistry of Materials, 2008, 20, 5675-5681.) One could imagine attempting to prepare Ba2In5P5 by the following reaction: 2BaBr2 + 6 InP → Ba2In5P5 + InBr + PBr3 (Note: All of these compounds are real, but the reaction is hypothetical.) The following molar masses might come in handy: BaBr2 297.14; InP 145.79; Ba2In5P5 1003.61; all units are g/mol.   a) Suppose the reaction is carried out with 110 g of BaBr2 and 210 g of InP. What is the limiting reagent?        b) How much (mass in grams) Ba2In5P5 would you make if the reaction went to completion?    c) After isolating and purifying the product, you only obtained 56 g of Ba2In5P5. What was your percent yield?

Antimony reacts with sulfur according to this equation. 2Sb(s) + 3S(s) → Sb2S3(s) What is the percentage yield for a reaction in which 1.40 g of Sb 2S3 is obtained from 1.73 g of antimony and a slight excess of sulfur? a) 80.9% b) 58.0% c) 40.5% d) 29.0%

When 4.50 g of Fe2O3 is reduced with excess H2 in a furnace, 2.60 g of metallic iron is recovered. What is the percent yield? This is the equation representing the reaction. Fe2O3 has a molar mass of 159.7 g x mol-1 Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H2O (g) a) 82.6% b) 70.0% c) 57.8% d) 31.5%

If 12.362 g of nitrogen is allowed to react with 4.133 g of hydrogen at 49.05 oC and the percent yield for the reaction is 55.61% , how much ammonia would be produced? The reaction proceeds as follows: N2 (g) + 3 H2 (g) → 2 NH3 (g) A. 8.361 g B. 12.93 g C. 15.04 g D. 23.24 g E. 6.856 g    

Lithium nitride, Li3N is an interesting salt. It is a fast ion conductor and it has also been studied as an anode material for batteries. Lithium nitride is produced according to the following reaction: 6 Li (s) + N 2 (g) → 2 Li3N (s) If the percent yield of the reaction at 85.00 oC is 65.28% and the reaction yields 18.326 g of lithium nitride from an experimental quality of lithium, how much lithium nitride would theoretically be expected in the experiment? A. 3.560 g B. 11.96 g C. 28.07 g D. 27.89 g E. 18.25 g

When octane (C8H18) is burned in a particular internal combustion engine, the yield of products (carbon dioxide and water) is 93%.  What mass of carbon dioxide will be produced in this engine when 15.0 g of octane is burned with 15.0 g of oxygen gas?  A)  13 g               B)  12 g                C)  21 g                 D)  54 g               E)  43 g

Under certain conditions the reaction of 64.00 grams of oxygen with excess nitrogen monoxide produced 92.0 grams of nitrogen dioxide.  What is the % yield of nitrogen dioxide in this reaction?   a. 25 % b. 50 % c. 100 % d. 12.5 % e. 64.00 grams of oxygens cannot produce more than 46.00 grams of nitrogen dioxide.  

Magnesium 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, theoretical yield and percent yield for the reaction. 

When heated, lithium reacts with nitrogen to form lithium nitride6 Li(s) + N2(g) → 2 Li3NWhat is the theoretical yield of Li3N grams when 12.3 g of Li are heated in excess N 2 ? ___________g What is the percent yield of the reaction if the actual yield of Li3N is 5.89g ?____________% 

Ammonia, NH3, reacts with hypochlorite ion, OCI -, to produce hydrazine N2H4. How many moles of hydrazine are produced from 5.85 mol of ammonia if the reaction has a 78.2% yield?2 NH3 + OCl- → N2H4 + Cl- + H2Oa) 2.29 molb) 2.92 molc) 4.57 mold) 9.15 mol

Ammonia, NH3, reacts with the hypochlorite ion, OCl - to produce hydrazine, N2H4.2NH3 + OCl – → N2H4 + Cl – + H2OWhat is the percent yield of hydrazine when 5.85 g of NH 3 reacts with excess hypochlorite to produce 2.60 g of N2H4? Molar mass: NH3 = 17.031 g/mol; N2H4= 32.046 g/molA. 47.3%B. 23.6%C. 11.8%D. 8.25%

DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction:     2C 6H5Cl      +    C 2HOCl3     →    C14H9Cl5    +   H2Ochlorobenzene         chloral                   DDT In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral.d. If the actual yield of DDT is 200.0 g, what is the percent yield?

Bornite (Cu3FeS3) is a copper ore used in the production of copper. When heated, the following reaction occurs:2Cu3FeS3(s) + 7O2(g) → 6Cu(s) + 2FeO(s) + 6SO2(g)If 2.50 metric tons of bornite is reacted with excess O 2 and the process has an 86.3% yield of copper, what mass of copper is produced? 

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react with excess Al according to the following reaction. (Molar masses: Fe = 55.85 g/mol, O = 16.00 g/mol, Fe2O3 = 159.70 g/mol)Fe2O3 (s) + 2 Al (s)  →  Al 2O3 (s) + 2 Fe (s)A. 61.03 %B. 28.65 %C. 57.30 %D. 20.02 %E. 81.93 %

Antimony reacts with sulfur according to this equation.2Sb(s) + 3S(s) → Sb2S3(s)What is the percentage yield for a reaction in which 1.40 g of Sb 2S3 (molar mass 339.7 g/mol) is obtained from 1.73 g antimony (molar mass 121.8 g/mol) reacting and a slight excess of sulfur (molar mass 32.07 g/mol)?A) 80.9%B) 58.0%C) 40.5%D) 29.0%

What is the percent yield of the reaction shown below if 29.6 g of gold (Au) are combined with 50.0 mL of 4.00 M HOCl (M = 54.46) in the presence of excess HCl, and 33.9 g of AuCl3 (M = 303.32) are obtained as a product? Enter your answer with 2 decimal places and no units.2Au(s) + 3HCl(aq) + 3HOCl(aq) → 2AuCl3(s) + 3H2O(l) 

The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between sodium bicarbonate and citric acid, C6H8O7:3NaHCO3 (aq) + C6H8O7 (aq) → 3CO2 (g) + 3H2O (l) + Na 3C6H5O7 (aq)If 1.00 g of sodium bicarbonate and 1.00 g of citric acid are allowed to react, what is the limiting reagent?  How many grams of carbon dioxide can theoretically form? How much of the excess reagent is left over after the reaction has come to completion? If you perform the experiment with an actual yield of 0.49 g, what is your percent yield for the reaction?

Sulfur dioxide (SO2) was prepared by reacting 13.2 g of sulfur and 5.0 g of oxygen. Calculate the percent yield of the reaction if 0.10 moles of SO2 were obtained from the reactionS + O2 → SO2   

Consider the general chemical equation:3A → 2BAssume that you start with 120.0 g of substance A and you eventually isolate 22.0 g of substance B. If you know that the molar mass of A is 60.0 g mol-1 and the molar mass of B is 33.0 g mol-1, find the % yield of the reaction.  

Combining 0.254 mol of Fe2O3 with excess carbon produced 12.8 g of Fe.Fe2O3 + 3C → 2Fe + 3COa) What is the actual yield of iron in moles?b)What was the theoretical yield of iron in moles?c)What was the percent yield?

When ethane (C2H6) reacts with chlorine (Cl2), 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 106 g of C2H6 reacts with 247 g of Cl2, assuming that C2H6 and Cl2 react only to form C2H5Cl and HCl. B) Calculate the percent yield of C2 H5 Cl if the reaction produces 181 g of C2 H5 Cl.

In the following reaction, the theoretical yield of Fe was calculated to be 105 g. If the actual yield was 87.9 g, what was the percent yield?Fe2O3 + 3CO → 2Fe + 3CO 2a) 65.3 %b) 83.7 %c) 112 %d) 97.8 %e) 59.0 % 

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H2O (I) → Ca(OH)2 (s) In a particular experiment, a 1.50-g sample of CaO is reacted with excess water and 1.48 g of Ca(OH)2 is recovered. What is the percent yield in this experiment? Select one: a. 99 b. 74.8c. 0.99 d. 101.2 e. 2.16 

Assuming an efficiency of 30.60%, calculate the actual yield of magnesium nitrate formed from 140.2 g of magnesium and excess copper (II) nitrate.Mg + Cu(NO3)2 → Mg(NO3)2 + Cu

Consider the reaction shown below:   3 H2(g) + N2 (g) → 2 NH3 (g)When a certain amount of hydrogen reacts in excess nitrogen, it produces 2.153 g of ammonia with a percent yield of 38.25%, what is the theoretical yield?A) 5.629 gB) 0.1778 gC) 0.8235 gD) 0.05701 gE) 7.768 g

Sodium and nitrogen combine to form sodium nitride;6Na(s)+N2(g) → 2Na3N(s)a) if 80.0 g of sodium is mixed with 20.0 g of nitrogen gas, what mass sodium nitride forms?b) If the reaction in part "a)" has a percent yield 75.0%, how much sodium nitride is actually produced?

Part A: What is the theoretical yield of ethyl chloride in the reaction of 19.6 g of ethylene with 50 g of hydrogen chloride? (For ethylene, MW = 28.0 amu; for hydrogen chloride, MW = 36.5 amu; for ethyl chloride, MW = 64.5 amu.)H2C=CH2 + HCl → CH3CH2ClPart B: What is the percent yield if 27.5 g of ethyl chloride is actually formed?

Each step in the process below has a 90.0% yield.CH4 + 4Cl2 → CCl4 + 4 HClCCl4 + 2 HF → CCl 2F2 + 2 HClThe CCI4 formed in the first step is used as a reactant in the second step. If 4.50 mol of CH  4 reacts, what is the total amount of HCl (moles) produced? Assume that Cl2 and HF are present in excess.

A 14.579 g sample of CaCl2 was added to 12.043 g of K2CO3 and mixed in water. A 3.531 g yield of CaCO3 was obtained. What is the limiting reagent? Calculate the percent yield of CaCO3.

Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide.4HCl(aq) + MnO2(s) → MnCl2(aq) + 2H2O(l) + Cl2(g) You add 35.5 g of MnO2 to a solution containing 42.5 g of HCI. (a) What is the limiting reactant?  (b) What is the theoretical yield of Cl 2 in grams? (c) If the yield of the reaction is 71.1%, what is the actual yield (grams) of chlorine?

Hydrazine, N2H4, may react with oxygen to form nitrogen gas and water. N2H4(aq) + O2(g) → N2(g) + 2H2O(I)If 3.65 g of N2H4 reacts and produces 0.650 L of N2, at 295 K and 1.00 atm, what is the percent yield of the reaction? 

Hydrazine, N2H4, may react with oxygen to form nitrogen gas and water. N2H4 (aq) + O2(g) → N2 (g) + 2H2O (l) If 3.25 g of N2H4 reacts and produces 0.650 L of N2, at 295 K and 1.00 atm, what is the percent yield of the reaction?

An iron nail rusts when exposed to oxygen. For the following reaction,  5.71 grams of iron are mixed with excess  oxygen gas. The reaction yields 7.36 grams of  iron(III) oxide. iron (s) + oxygen (g) → iron(III) oxide (s) a) What is the theoretical yield of  iron(III) oxide? b) What is the percent yield for this reaction ?

Tetraphosphorus hexoxide is formed by the reaction of phosphorus with oxygen gas. If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of tetraphosphorous hexoxide, what is the percent yield for the reaction? (Please show all steps and methods).