4. What is one reason that a person might get more than 100% yield?

Q: Gaseous methane (CH,) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO,)…

A: Given :-  Amount of methane  = 4.7 g  Amount of oxygen gas = 6.1 g  Actual yield of carbon dioxide…

Q: Consider the hypothetical reaction shown here. If 11 mol of A combine with 16 mol of B and the…

A: Limiting reagent: It is defined as the reactant in a chemical reaction which is present in lesser…

Q: For the following reaction, 0.308 moles of hydrogen gas are mixed with 0.189 moles of ethylene (C2…

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Q: 10.0 grams of methane is burned in an excess of oxygen and the reaction forms 19.8 grams of water in…

A: The percentage yield of a product in a reaction is the percentage of that product obtained compared…

Q: 2 Mg(s) + 3 N2 (g) --> 2 MgN3 (s) How many moles of N2 will be used to produce 115 grams of MgN3?

A: The given reaction is,             2 Mg(s) + 3 N2 (g) --> 2 MgN3 (s) We have, mass of MgN3 = 115…

Q: What is the importance of calculating % yield of a reaction?

A: Percentage yield is given by the ratio of actual yield to that of the theoretical yield multiplied…

Q: What mass of N2 is needed to produce 10.00 g N3F? 3N2 + F2 ⎯→ 2N3F

A: Number of moles present in 10.00 g N3F is determined as shown below: No.of moles=massMolar massNo.of…

Q: d. How much excess reactant is left over after the reaction is complete? (5.84) e. What is the…

A: As., You solved the first three part of the question  I solve other two part of question in step 2.…

Q: 19 g of H2S with excess O2 produced 8 g of sulfur. ? H2S + ? O2 → ? S + ? H2O . What is the percent…

A: Mass of H2S = 19 g  Actual yield of S = 8 g. Percentage yield of Sulfur = ?

Q: Why is the actual yield in a reaction almost always less than the theoretical yield? (c) Can a…

A: The ratio of actual yield to the theoretical yield multiply by 100 is known as percentage yield.

Q: A) How many grams of water can you produce if you have 25.0 grams of H2 and 50.0 grams of O2?  B)…

A: Limiting Reagent is the reactant which is completely consumed when a reaction goes to completion.

Q: 5. Benzene, C&H6, has a density of 0.787 g/mL. Burning 10.0 mL of benzene would produce how many…

A:

Q: The combustion of propane (C3H8) produces CO₂ and H₂O: C3H8 (g) +502 (g) -> 3CO₂ (g) + 4H₂O(g) The…

A:

Q: Consider the following unbalanced reaction: P4 (s)+F2(g)→ PF3 (g) What mass of F2 is needed to…

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Q: 3.87 Why is the actual yield of a reaction almost alwayssmaller than the theoretical yield?

A: The chemical reaction is the one in which the reactants will be converted into the products. The…

Q: Fe,03 + HCI → FeCl, + H2O 5 g 5 g ?g 5. How many grams of the product is produced?

A:

Q: In the lab, 9.00 g of hydrogen, H2, is reacted with excess oxygen gas, O2, and 73.0 g of water is…

A:

Q: What factors during the experiment caused the percent yield to be different than 100%? What…

A: Interpretation: To spot the impurities in the IR data of the product i.e. cyclohexene. The…

Q: Consider the combination reaction: 2 Al(s) + 3 Br2(1) 2 AIBr3(s) ----> Suppose the actual yield of…

A: We have to predict the theoretical yield.

Q: Define the terms theoretical yield, actual yield, and percentyield. (b) Why is the actual yield in a…

A: (a) Theoretical yield could be defined as the maximum amount of products which could be formed from…

Q: Which of the following statements is false? A) Actual Yield Theoretical Yield The percent yield = B)…

A: Given Statements  The percent yield = Actual yieldTheoretical yield * 100yes This satatement is true…

Q: Glucose (C6H12O6) reacts with excess oxygen to produce 150 g water. ?^?KE?^ + ?E → ??E + ?E? a)…

A: Glucose reacts with water to produce carbon dioxide and water as per the reaction  C6H12O6 + O2…

Q: Question attached

A: Number of moles of the substance is equal to the ratio of mass to the molar mass of the substance.…

Q: Chemistry The reaction between NH3 and Br2 produces N₂Br4 and HBr. What number of molecules of N₂Br4…

A:

Q: 8. What could a 101% percent yield mean? A. The reaction was a success. C. It was a perfect chemical…

A: By definition, % yield is calculated as: % yield = Actual yieldTheoretical yield×100 where Actual…

Q: When nitrogen gas and hydrogen gas are mixed at 350°C and a high pressure, they react to form 28.96…

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Q: (CH,(CH),CH,) Gaseous butane (CH. reacts with gaseous oxygen gas (0,) to produce gaseous carbon…

A: Given :-  amount of CH3CH2CH2CH3 = 1.7 g  amount of O2 = 4.7 g  To calculate :-  theoretical yield…

Q: d. What is your theoretical yield of BeH2 in moles? e. What is your theoretical yield of BeH₂ in…

A:

Q: 5. Consider the following reaction: NazPOa(aq) + Ba(NO3)2(aq) → Ba3(PO.)2(s) + NANO3. Suppose a…

A: Since you have asked multiple questions, we will solve the first question (Question number 5) for…

Q: 2 C8H10 + 21 O2 ------------> 16 CO2 + 10 H2O   How many grams of O2 are required to produce 7.00…

A:

Q: 2 N2O5 ----> 4 NO2  +  O2 What mass of NO2 can be produced from the complete reaction of 38.2 g of…

A: Given  Reaction   2N2O5  → 4NO2  +  O2 Mass of N2O5   = 38.2 gram  Mass of NO2     = ?

Q: For the following reaction, 6.21 grams of methane (CH4) are allowed to react with 27.6 grams of…

A: The maximum amount of dichloromethane (CH2Cl2)is to be calculated The amount of the excess reagent…

Q: Suppose

A: Welcome to bartleby! Actual yield = 43.7 g  Theoretical yield = 56.0 g

Q: ? SO2 (g) +? O2 (g) → ? SO3 (g) Calculate the number of grams of SO2 that must react to produce…

A: Note: As per the guidelines, solution of first question has been made. For the expert solution of…

Q: 1. Magnesium metal reacts quantitatively with oxygen to form magnesium oxide, MgO. a. Write a…

A: The reaction of Magnesium metal with oxygen is an example of combustion reaction.

Q: Consider the following unbalanced chemical equation. C5H12(1) + O2(g) → CO2(g) + H20(1) If 19.2…

A: Recall, the unbalanced chemical equation,   C5H12 (l)  +  O2 (g)                    CO2 (g)  +…

Q: Is it possible for the calculated percent yield to be greater than 100% in the synthesis of alum?…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: 11. When 6.00 mole of BaCl, (aq) is mixed with .250 mole of K,AsO, (aq), what is the theoretical…

A:

Q: Lithium and nitrogen react in a combination reaction to produce lithium nitride:  6Li (s) + N 2 (g)…

A: Given :  6Li (s) + N 2 (g) → 2Li 3N (s)

Q: A reaction has a theoretical yield of 45.8 g. When the reaction is carried out, 37.2 g of the…

A: In a chemical reaction, yield is the estimation of the amount of the resultant compound synthesized.…

Q: 3 Mg   +   2 AlCl3   →   3 MgCl2   +   2 Al When this reaction was performed in the lab, 2.8 g of…

A:

Q: 2. What is the actual yield of the product?

A: Actual yield is  defined as the amount of a product that is formed from a chemical reaction

Q: 6. 45.2 g of Iron metal reacts with excess oxygen gas to produce 58.1 g of Fe3O4. a) What is the…

A: We need to calculate  Theoretical yield Percentage yield Actual yield

Q: b. 57% IG9 32g Given the reaction: CH+ 202 --> CO2 + 2H2O 45.5 When 16 g of methane (CH4) and 32 g…

A: Given - CH4 + 2O2--> > CO2+2H2O Mass of CH4=32 g Mass of O2=32g Mass of CO2=11g

Q: 4. 1 Nacl + 1 AgNO, → 1 AgCl + 1 NANO3 (a) 78.00 g of NaCl should produce how many grams of AgCl?

A: Solution: The given chemical equation is as follows --- 1 NaCl + 1 AgNO3 = 1 AgCl + 1 NaNO3…

Q: Hydrocarbon mixtures are used as fuels. What mass of CO2 gas is produced by the combustion of 343.5…

A: The mass of carbon dioxide produced by combustion of 50.8 % methane is calculated as,

Q: How many grams of H2 are required to produce 7.50 grams of ammonia NH3?  Use the balanced equation…

A: The balanced Chemical Reaction is - N2(g)+3H2(g)⟶2NH3(g) According to the balanced Chemical Reaction…

Q: In the reaction Benzoin → Benzil 5.6 g Benzil was produced with a Percent Yield of 66 % What is the…

A: Given data: Mass of Benzil produced = 5.6 g Percent yield = 66% Formula used: Percent Yield=Actual…

Q: The combustion of propane (C3H8) produces CO2 and H2O: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)…

A: