If the actual mass of a product formed in a reaction is 12.75 g less than the theoretically predicted mass of 25.69 g, what is the percent yield of this reaction? ?

Q: If 15.3 g of a particular product were obtained in a reaction and the theoretical amount was…

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Q: The theoretical yield of aluminum is 1.16 moles. If only 1.03 moles of aluminum were collected, what…

A: Given, Theoretical yield = 1.16 moles Actual yield = 1.03 moles % yield = ?

Q: In an experiment, 5.25 g of H2 was added to react with 12.5 g of O2. This produced 13.5 g of H2O.…

A: Given that, Mass of H2 = 5.25 g,  Molar mass = 2 g mol-1 Mass of O2 = 12.5 g, Molar mass = 32 g…

Q: When NH3 is prepared from 28g N2 and excess H2, the theoretical yield of NH3 is 34 g. When this…

A: For the reaction of N2 and H2 to form ammonia NH3 Given: Mass of N2=28 g  Theoretical yield of…

Q: For the following reaction, 0.400 grams of hydrogen gas are allowed to react with 54.7 grams of…

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Q: If 4.30 g of product was found at the end of a chemical reaction, but 7.20 g of product was…

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Q: When 3.16 g of N2 is allowed to react with an excess of Li2O, 1.28 g of Li3N are produced. What is…

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Q: Suppose the theroretical ye old in a reaction is 10.5 g and the percent yield is 75.5 percent. What…

A: Theoretical yield =10.5 g percent yield=75.5 g Percent Yield=Actual Yield/ Theoretical Yield×100%…

Q: Methane (CH,) is the main component of marsh gas. Heating methane in the presence of sulfur produces…

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Q: A 1.00-g sample of potassium bicarbonate is decomposed by heating. If the resulting potassium…

A: Given details, The balanced chemical equation, 2KHCO3 → K2CO3 + CO2 + H2O The actual yield = 0.725 g…

Q: A sample of 42.9 g MnO, is added to a solution containing 41.3 g HCl. What is the limiting reactant?…

A: number of moles = mass/molar mass  mass = moles × molar mass  percent yield ={actual…

Q: (a) Define the terms limiting reactant and excess reactant.(b) Why are the amounts of products…

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Q: Once the reaction has occurred as completely as possible, what amount (in moles) of the excess…

A: The given chemical equation is perfectly balanced. 2 moles of ZnS requires 3 moles of O2, then 1…

Q: Your theoretical yield is 63.247 g. You isolated 13.5648 g of alum. What is your percent yield?

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Q: The percent yield for a given reaction is 47%. If the theoretical amount is predicted to be 5.29 g,…

A: Formula for calculating percent yield: Percent yield = 100 x Actual yield/Theoretical yield

Q: An excess of oxygen reacts with 451.4 g of lead, forming 366.9 g of lead(II) oxide. Calculate the…

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Q: A 0.4011 g sample of aluminum reacts according to our experiment to produce alum. 5.7968 g of dried…

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

Q: The combustion of 0.374 kg of methane in the presence of excess oxygen produces 0.983 kg of carbon…

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Q: Determine the limiting reactant, theoretical yield of C7H1807 (g), and percent yield for the…

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Q: The percent yield for a given reaction is 75%. If the theoretical amount is predicted to be 3.58g,…

A: Percent yield of the reaction is equal to the ratio of actual yield and theoretical yield multiplied…

Q: For the following reaction, 0.367 moles of carbon disulfide are mixed with 0.540 moles of chlorine…

A: The question is based on the concept of reaction stoichiometry. a limiting reagent is the reagent…

Q: For the following reaction, 4.70 grams of hydrogen gas are allowed to react with 43.0 grams of…

A: Given, mass of hydrogen (gas) = 4.70 gmass of iodine (solid)    =43.0 g

Q: If 45 grams of N2 are actually determined from a reaction, what is the percent yield if the…

A: Percent yield is defined as the percentage ratio of the actual yield to the theoretical yield…

Q: Consider the reaction of CO2 with KOH to form K2CO3 and H2O. If 3.23 g KOH is reacted with excess…

A: The chemical reaction between KOH and CO2 is 2KOH(aq) + CO2(g)—-----> K2CO3(aq) + H2O(aq)First,…

Q: A 0.4505 g sample of aluminum reacts according to our experiment to produce alum. 5.7955 g of dried…

A: Given : Mass of Al reacting = 0.4505 g And mass of Alum produced = 5.7955 g Molecular formula of…

Q: An experiment involving 12 grams of carbon is mixed with 64 grams of oxygen causing the production…

A: We have to predict the limiting reactant and excess reactant.

Q: What is the percent yield if the combustion of gasoline results in 680 grams of steam produced when…

A: Given, theoretical yield of steam = 985 g. Actual yield of steam = 680 g. We have to calculate the…

Q: A 1.897 g sample of pure Mg(HCO3)2 was heated and decomposed. When the sample cooled, it weighed…

A: Any reaction's percent yield gets computing by taking ratio of its actual yield with its calculated…

Q: When 6 moles of H₂ reacted with 3 moles of N₂ to produce, NH₃, which is the limiting reactant? *

A: Answer: In chemical reaction, limiting reagent is the reactant that exhausted first and decided the…

Q: For the following reaction, 3.76 grams of hydrogen gas are allowed to react with 40.5 grams of…

A: Part 1:  The maximum Mass of HI produced is 40.82g Part 2:  Molecular formula for limiting reagent…

Q: If 25.0 g potassium metal are reacted with 25.0 g oxygen gas to yield 22.37 g potassium oxide, what…

A: A numerical problem based on mole concept, which is to be accomplished.

Q: Tests are to be conducted on a new anti-cancer drug and you are to prepare a fresh supply for the…

A: Actual Yield = 1.345 g Theoretical Yield = 1.433 g So, Percent Yield = (Actual Yield / Theoretical…

Q: Suppose that in the synthesis of isoamyl acetate, a student began with 6.209 grams of acetic acid…

A: The theoretical yield of the reaction is calculated as,

Q: my theoretical yield was 45.0g. If my percent yield was 68.0%, how much was my actual yield?

A: Since we know that  Percent yield = (actual yield / theoretical yield )×100%  So by using this…

Q: Consider the following unbalanced equation for the combustion of pentane: if a 20.4 g sample of…

A: Given that 20.4 g pentane react with excess oxygen.

Q: For the following reaction, 6.52 grams of sulfuric acid are mixed with excess barium hydroxide. The…

A: Given :-  amount of sulfuric acid = 6.52 g  actual yield of barium sulfate = 11.7 g  To be…

Q: 1.51 grams of H2 is allowed to react with 10.2 grams of N2, producing 1.34 grams of NH3. What is the…

A: Given that  Mass of H2  = 1.51 g Mass of  N2 = 10.2 g Mass of NH3  (Actual yield)= 1.34 g Percent…

Q: c) How many grams of the excess reactant remain after the limiting reactant is completely consumed?…

A: limiting reagent is completely consumed in a reaction, the maximum amount of yield that is the…

Q: According to the following reaction, how many moles of bromine monochloride will be formed upon the…

A: Given: Mass of Br2 = 32.8 g Molar mass of Br2 = 159.808 g/mol

Q: In a reaction to produce ammonia, the theoretical yield is 420.0 g. What is the percent yield if the…

A: Percent yield of the reaction is equal to the ratio of actual yield and theoretical yield multiplied…

Q: According to the following reaction, how many grams of calcium oxide will be formed upon the…

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Q: For the following reaction, 5.33 grams of hydrogen gas are allowed to react with 47.7 grams of…

A: Given,

Q: If 68.0 g of sodium hydroxide and 44.0 g of carbon dioxide are allowed to react, which is the…

A: Mass of NaOH = 68.0g Mass of CO2 = 44.0g The reaction between NaOH and CO2 takes place. We have to…

Q: 56 grams of iron (III) sulfate reacts with 24 grams of lead (IV) nitrate a. Calculate the mass of…

A: As per our company guidelines we are supposed to answer only first three sub-parts. kindly repost…

Q: If the yield of the picric acid synthesis reaction is 65% what mass of picric acid what mass will it…

A: The synthesis of picric acid reaction is as follows,

Q: If 25.0 g potassium metal are reacted with 25.0 g oxygen gas to yield 17.98 g potassium oxide, what…

A: 4K + O2 ---> 2K2O Mass of K2O formed by 25 g of potassium metal  = 25 g K × (1 mol K/39.0983 g K)…

Q: Barium and phosphorus react with each other in a synthesis reaction. If 0.2856 g of phosphorus…

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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.