If the yield of the reaction is 76.7%, what is the actual yield of chlorine?

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: If the combustion of 83.22 g of C4H10 produced 52.68 g of CO2 what is the percent yield for this…

A:

Q: What is the theoretical yield (in grams) of potassium chloride when 2.500 grams of potassium metal…

A: Potassium metal reacts with chlorine gas to produce potassium chloride.  The mass of potassium is =…

Q: When HgO is heated, it decomposes into elemental mercury and diatomic oxygen gas. If 57.0 g of Hg is…

A: Given: Mass of HgO = 81.5 g Mass of Hg (actual yield) = 57.0 g/mol Molar mass of HgO = 216.59 g/mol…

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

A:

Q: What is the percent yield for a given process, if 4 kg of a product is recovered from a reaction…

A: formula to calculate  percent yield is , The percent yield=Actual yieldTheoretical Yield ×100  %

Q: 1.51 g H2 is allowed to react with 10.0 g N2, producing 2.01 g NH3. Part A What is the theoretical…

A: Mass of H2 = 1.51 g Mass of N2 = 10.0 g Mass of ammonia = 2.01 g

Q: What is the percent yield of a reaction if it had a theoretical yield of 125g but an actual yield of…

A: The equation for percent yield is: percent yield = (actual yield/theoretical yield) x 100% Where:…

Q: The combustion of 374 g of methane (CH,) in the presence of excess oxygen (O,) produces 983 g of…

A: The burning of a compound in excess of air or oxygen is called combustion . The chemical reaction…

Q: If the percent yield for a reaction is 100% and the theoretical yield is 88 g. What is the actual…

A: Actual yield is defined as quantity of a product received from a chemical reaction.

Q: Ammonia reacts with diatomic oxygen to form nitrogen monoxide and water vapor: NH3 +          O2…

A: The reaction taking place is given as, => NH3 + O2 ------> NO + H2O Given: Mass of NH3 taken =…

Q: What is the percent yield for the reaction of nitrogen and hydrogen to produce ammonia, if the…

A: We have the equation for calculating percent yield as follows % yield=Actual yieldTheoretical yield…

Q: If the theoretical yield of a reaction is 0.102 gg and the actual yield is 9.40×10−2 gg , what is…

A:

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: A mixture of 10.0 g of NO and 14.0 g of NO2 results in the production of 8.52 g of N2O3. a.) Give…

A: Every reactant molecule reacts in a specific stoichiometric ratio to form the product. The balanced…

Q: A reaction has a theoretical yield of 55.8 g. When the reaction is carried out, 37.2 g of the…

A: Percent yield is the percent ratio of actual yield to the theoretical yield. It is calculated to be…

Q: The theoretical yield of a reaction is 75.0 grams of product and the actual yield is 42.0 g. what is…

A: Given as The theoretical yield of a reaction is 75.0 gram and actual yield is 42.0 g % yield has to…

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: Consider the mixture of propane, C3H8, and O2 shown here.(a) Write a balanced equation for the…

A: a. C3H8 + 5O2 ---------------> 3CO2 + 4H2O

Q: The reaction of 421.3 g of TiO, with excess H2 yields 325.2 g of TiżO3. Calculate the theoretical…

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

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: Consider the reaction Al (s) -3 F, (g) -→ 2 AIF, (s) If 85.43 g of aluminum reacts with 85.43 g of…

A:

Q: The reaction of 6.85g of carbon with O2 yields 9.30g of CO2. What is the percent yield of this…

A: The reaction is written below. C + O2 → CO2 The molar mass (M) of carbon is 12.01 g/mol .The number…

Q: Calculate the percent yield of a reaction if the theoretical yield of the reaction is 1.43 moles,…

A: ans: 80.41% % yield = Actual yield /theoretical yield x 100 given theoretical yield=1.43 moles…

Q: What is the theoretical yield of boron when 2350g of boric oxide is reacted with 3580g of magnesium?…

A: Step : 1             What is the theoretical yield of boron ?

Q: what is the percent yield?

A: The ratio between the actual yield and the theoretical yield multiply by 100 is known as percent…

Q: Consider the reaction of solid P₄ and chlorine gas to form gaseous phosphorus trichloride. The…

A: Percent yield of any reaction is given in terms of product as

Q: How many moles of NH, can be produced from 2.61 moles of nitrogen in the following reaction: N, (g)…

A: Balanced Reaction N2 (g) + 3 H2 (g) ---> 2 NH3 (g) N2 reacts with hydrogen molecule to form…

Q: 3H2(g)+N2(g)→2NH3(g) 1.86 g H2 is allowed to react with 9.74 g N2, producing 1.69 g NH3. a) What is…

A: Limiting reagent is the reactant that limits the chemical reaction and determines the amount of the…

Q: How many grams of hydrogen, H2, are produced from 29.3 g of aluminum, Al?

A: Given Synthesis of H2 from Al

Q: What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of…

A: Given :  Al + Cr2O3 → Al2O3 + Cr  Amount of Al = 8.00 g  Amount of Cr2O3 = 40.0 g  To calculate :…

Q: If you had excess aluminum, how many moles if aluminum chloride could be produced from 27.0 g of…

A: Given:Mass of Cl = 27.0gMolar mass of chlorine atom, Cl = 35.45Molar mass of chlorine molecule, Cl2,…

Q: reaction has a theoretical yield of 76.5 grams of a product, and a percent yield of 41.2  %.  What…

A: The question is based on the concept of reaction calculations. we have to calculate actual yield of…

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: In a certain reaction between CO and Fe3O4, the theoretical yield of Fe is calculated to be 47.2g.…

A: The percent yield is unique way that gets utilized in depicting the reactant’s quantity that…

Q: If a reaction that produces CO2 had a theoretical yield of 19.4 g and it actually produced 15.0 g of…

A: The percent yield has to be calculated,

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: If 5.3 g of hydrogen gas is reacted with 12.6 g of oxygen gas to produce water, which reactant is…

A: Given, mass of hydrogen = 5.3 g mass of oxygen = 12.6 g

Q: What is the theoretical yield of iron in grams if 67 g of CO are reacted with 72 g of Fe2O3?…

A: We have to first calculate limiting reagent.

Q: Assume that you have an unlimited amount of water, how many grams of hydrogen are produced if 300.00…

A: write down the balanced equation first,2 Na + 2 H2O →2 NaOH + H2   Given that,mass of Na that…

Q: When 65.0 g of benzene (C,H6) burns in oxygen to give 32.9 g carbon dioxide and water are formed, if…

A: Given :-  Mass of C6H6 = 65.0 g  Mass of CO2 = 32.9 g  Theoritical yield = 35.5 g  To be calculated…

Q: If 15.0 g potassium metal are reacted with 15.0 g oxygen gas to yield 14.3 potassium oxide, what is…

A: Reaction occurs as: Moles can be given as: n: Number of moles. m: Mass of the reactants or…

Q: Copper (I) sulfate is produced when copper is heated with sulfur.  If 1.5 g of Cu was heated with an…

A: Given: Mass of Cu = 1.5 g Mass of Cu2SO4 = 1.76 g Molar mass of Cu = 63.546  g/mol Molar mass of…

Q: In an experiment, 3.250 g of NH3 reacted with 3.50 g of O₂. Supposed that the reaction produced 2.13…

A: We have given that  In an experiment 3.250 g of NH3 reacted with 3.50 g of O2 Supposed that the…

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: Assume that the theoretical yield of iron in the process  was 47.6 g. 3Ba(s) +Fe2O3(s) arrow 3BaO…

A: The answer to the following question is given as:

Q: 25.0 g potassium metal are reacted with 25.0 g oxygen gas to yield 12.45 g potassium oxide, what is…

A:

Q: In the reaction involving 2.6 g of lead (II) nitrate and 4.6 g of potassium bromide, what is the…

A:

Q: 1.65 g H2 is allowed to react with 10.0 g N2, producing 1.79 g NH3. What is the theoretical yield in…

A: The reaction between H2 and N2 is as follows,

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.