When heated, lithium reacts with nitrogen to form lithium nitride: 6Lİ«) + Nz«g) → 2Lİ3N«) (a) What is the theoretical yield of Li3N in grams when 12.3 g of Li are heated with 33.6 g of N2? (b) If the actual yield of Li3N is 5.89 g, what is the percent yield of the reaction?

Q: What is the theoretical yield of water in grams if 6.3 grams of propane, C3H8, is burned?

A: Given -> Weight of propane = 6.3 gm

Q: Consider the reaction: 2Na(s) + Cl₂(g) → 2NaCl(s) A student is making sodium chloride (NaCl(s)) by…

A: we have to calculate the percentage yield

Q: When 65.0 g of benzene (C6H6) burns in oxygen to give 32.9 g carbon dioxide and water are formed, if…

A: Given : Mass of C6H6 reacted = 65.0 g Mass of CO2 produced = 32.9 g And the theoretical yield of CO2…

Q: What is the mass in grams of H2 that can be formed from 54.6 G of NH3 in the following reaction? 2…

A: From the stoichiometry, we can easily calculate , the problem.

Q: If 5.9 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, how many kg of CO₂ is…

A: Calculate the moles of CO2 produced, Calculate the mass of CO2 produced,

Q: how is the answer 78.55%?

A: The two reaction are as follows:…

Q: The equation for the reaction between sodium hydrogen carbonate and sulfuric acid at room…

A:

Q: Take the reaction: NH3 + O2 ---> NO + H2O. In an experiment, 3.25 g of NH3 are allowed to react with…

A:

Q: Consider an example of a thermite reaction: 3 CuO(s)  +  2 Al(s)  →  3 Cu(s) +  Al2O3(s) When 5.00…

A: we have to calculate the percentage yield of the reaction

Q: Ethyl alcohol (C₂H5OH), also called grain alcohol, can be made by the fermentation of glucose:…

A:

Q: How many moles of lithium hydroxide would be required to produce 86.5 g of Li,CO3 in the following…

A:

Q: Nitrous oxide (N,0), also known as “laughing gas," is commonly used as an anesthetic in dentistry.…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: TiCl4 (189.68 g/mol), a source of Ti metal, can be produced from titanium dioxide, carbon and…

A:

Q: In a combustion reaction between 700.0 mL propane, C3H8 with oxygen gas, O2 at 25 °C, an unknown…

A: The chemical equations should be balanced in accordance with the law of conservation of mass.…

Q: 1. (a) For the double displacement reaction and find the mole ratio between the product and…

A: Double displacement reaction is a reaction in which exchange of ions occurs between the reactants to…

Q: The reaction of finely divided aluminum and iron(III) oxide, Fe2O3, is called the thermite reaction.…

A: Given,  Mass of Al = 500.0 g  Mass of Fe2O3 = 500.0 g  Mass of Fe produces = Actual yield of Fe =…

Q: The balanced equation for the reaction of aluminum metal and chlorine gas is 2AI(s) + 3Cl,(g) →…

A: The limiting reactant is the reactant which is totally consumed after the completion of the…

Q: In an experiment designed to produce calcium oxide by the chemical reaction: 2Ca + O2 → 2CaO…

A: Given reaction is,  2Ca + O2 → 2CaO Also Given is, 104.5 g of CaO was obtained out of a possible…

Q: What is the mass in grams of H₂ that can be formed from 70.4 grams of NH₃ in the following reaction?…

A: Given, 70.4 grams of NH₃

Q: 892.1 grams of isomaltitol, C12H24O11, was combusted in a furnace completely in an excess oxygen.…

A: The yield of water can be calculated as:-

Q: What is the mass in grams of magnesium chloride that can be produced from 6.68 moles of chlorine gas…

A: Given, Mg(s)+Cl2(g) ➝ MgCl2 moles of chlorine (Cl2) gas reacts = 6.68 moles Excess reactant ➝…

Q: Calculate each of the following quantities:(a) Mass in grams of 6.44x10^-2mol of MnSO₄(b) Moles of…

A: Number of moles of MnSO4 = 0.0644 mol Mass of MnSO4 is determined by multiplying the number of moles…

Q: The balanced equation for the reaction of aluminum metal and chlorine gas is 2Al(s) +…

A: To determine the limiting reactant and the maximum amount of AlCl3 that can be produced, we need to…

Q: Calculate the maximum amount in grams of H₂O that can be produced by the reaction of 550 mg of H₂…

A: Given, H2(g) + O2(g) ➝ H2O(g) Balancing the above equation: 2H2(g) + O2(g) ➝ 2H2O(g) Note: 1000 mg =…

Q: (b) What mass of Na,AlO, can be formed from 165.0 g of NaOH?

A:

Q: Balance the following chemical equation CB,H.(g) + O₂(g) - > CO₂(g) + H₂O(g)

A: Is an equation in which the number of atoms for each element in the reaction and the total charged…

Q: CH4(g) + 2 Cl2(g) → CH2C12(g) + 2 HCI(g) CH4 reacts with Cl2 as shown by the equation above. A…

A: (a) According to given balanced Chemical Reaction - 1 mole methane required = 2 mole of Chlorine…

Q: reaction product is produced in a 76.3% yield. If the actual yield of the isolated product is 31.1…

A: Percentage yield= (actual yield/theoretical yield)*100% Let m=theoretical yield 76.3 =(31.1/m)*100…

Q: The percent composition of an unknown substance is 46.43% C, 25.77% O, 18.05% N, and 9.74% H. What…

A:

Q: The synthesis of maleic acid anhydride (C₄H₂O₃) can be accomplished by reacting benzene (C₆H₆) and…

A: Balanced chemical equation   2 C₆H₆(l) + 9 O₂(g) → 2 C₄H₂O₃(s) + 4 CO₂(g) + 4 H₂O(g)

Q: Consider the following reaction: C3H8 + O2 → H2O + CO2. (a) Balance the reaction. (b) If you start…

A: We have a unbalanced equation , we have to balance it, Then we are having 100 g of each reactant ,we…

Q: The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is…

A: Given, mass of NO = 9.500 g Mass of O2= 11.99 g Molar mass of NO = 30.0 g/mol Molar mass of O2=…

Q: A sample of sodium carbonate, Na2CO3, weighs 40.0 g. Calculate the following quantities (a) ? mol…

A: The number of molecules or atoms present in the one mole of the substance is equal to the Avogadro…

Q: This question has multiple parts: The following equation represents the formation of water from…

A:

Q: Be sure to answer all parts. Propane (C3Hg) is a minor component of natural gas and is used in…

A: Part a)  given reaction :-   C3H8(g) + O2(g)  --->  CO2(g) + H2O(g)    Part b)   given moles of…

Q: Ammonia gas can be prepared by the following reaction: CaO(s) +2 NH,Cl(s) → 2 NH3 (g) + H, 0(g) +…

A: Given data :  Given mass of CaO = 184 g  Given mass of NH4Cl = 368 g  Theoretical yield of NH3= 112…

Q: When 12.0 g of carbon is burned in oxygen during an experiment, only 40.4 g of carbon dioxide was…

A: Weight of 1 mole of compound is called the molar mass of that compound.

Q: Chloroform, CHCl3, reacts with chlorine, Cl2, to form carbon tetrachloride, CCl4, and hydrogen…

A: Limiting reactant can be defined as the reactant that get totally consumed in the reaction and…

Q: How much (in gram) of HCl is required to produce 21.45 g of  AlCl3 if the percentage yield for the…

A: The balanced reaction taking place is given as, => 2 Al (s) + 6 HCl (aq) →2 AlCl3 (s) + 3 H2 (g)…

Q: 2 Cu + S→ Cu;S When copper is heated with sulfur, the reaction above takes place. If 100. g of Cu is…

A:

Q: In a reaction to produce NaF, 3.50 g of HF and 1.26 of Na2SiO3 are reacted according to the…

A: Consider the reaction: Na2SiO3 (s) + HF (aq) →H2SiF6 (aq) + NaF (aq) + H2O (l)  The mass of Na2SiO3…

Q: What mass of aluminum oxide can be produced from 100.0 g of aluminum given the reaction:  4Al (s) +…

A: By using mole-mole analysis in balanced reaction mass of Al2O3 can be calculated.

Q: The combustion of methane is shown in the following reaction:CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) A)…

A: Given information: Number of moles of CO2 gas produced = 15.0 mol Number of moles of O2 gas consumed…

Q: A sample of calcium metal with a mass of 2.00 was reacted with excess oxygen. The following equation…

A: Coefficients vs. Subscripts 4Anatomy of a Chemical EquationReactants appear on theleft side of the…

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.