1.15g sample of sodium reacts with 0.8g of sulfur to form sodium sulfide. (MM of Na = 23 g/mol and MM of S = 32 g/mol), MM = molar mass What is the mole ratio of sodium to sulfur in the sample? What is the empirical formula of the Sodium sulfide?

Q: Calculate how many grams of lead (II) iodide (MM=461.01 g/mol) can be formed from 1.385 g of sodium…

A: Given:Molar mass of PbI2  = 461.01gMolar mass of NaI  = 149.89gmass of NaI reacted = 1.385gAlso,The…

Q: A flask contains 0.470 mol of liquid bromine, Br2. Determine the number of bromine molecules present…

A: It is given that there is 0.470 mol of liquid bromine.

Q: Calculate the number of motes for 5.34 x10 molecules of Zinc. 25

A: Solution of question is given below.

Q: If 1.75 g of potassium iodide and 3.21 g of silver nitrate are combined, then what is the limiting…

A: First, we must examine the reaction stoichiometry. In this reaction, one mole of AgNO3 reacts with…

Q: You are given 0.10 g samples of Na, Y, Ge, and Mn. List the samples in order of the amount (moles)…

A: Number of moles = given mass/molar mass

Q: A flask contains 0.390 mol of liquid bromine, Br2. Determine the number of bromine molecules present…

A: Given, Number of moles = 0.390

Q: The Haber-Bosch process involves the combination of nitrogen and hydrogen at high temperatures in…

A: Production of ammonia depends on limiting reagent. Limiting reagent is completely used during the…

Q: Explain the problem with the following statement and correct it. “When a chemical equation is…

A: The given statement is to be corrected by explaining the error with it. The given statement is:…

Q: un o 8u described in this laboratory. After heating, the sample is found to weigh 2.245 grams. How…

A:

Q: 1 Bao + 1 H50, → 1 Bas0, + 1 H,0 3. (a) What mass of BaSO, can be formed from 196.0 g of H,SO,?

A: Use the stoichiometric calculations as shown below:

Q: The reusable booster rockets of the U.S. space shuttle employ a mixture of aluminum and ammonium…

A:

Q: A student was given a sample of hydrated Na2CrO4 (molar mass of anhydrous Na2CrO4: 162.0 g/mol). She…

A:

Q: What is the maximum amount of grams of Fe that can be produced from 33.4 g of iron(iii) oxide mixed…

A: Interpretation: The maximum amount of grams of Fe that can be produced from 33.4 g of iron(iii)…

Q: Oxides of virtually every element are known. Bromine, for example, forms several oxides when treated…

A: Given : Mass of Br2 reacting = 1.350 g And mass of BrxOy formed = 2.026 g Since the compound is…

Q: A 0.700 g sample of phosphorous is reacted with excess oxygen to form a product with a mass of 1.604…

A:

Q: What is the maximum mass of iron (III) chloride that can be produced from 25g iron (1II) oxide and…

A: 1) Reaction: Fe2O3+6HCl →2FeCl3+3H2O 2) Mass of Iron(III)oxide = 25 g 3) Mass of Hydrogen chloride=…

Q: A 0.613 g sample of a covalent compound contains 3.13 × 1021 molecules. What is the molar mass (in…

A: We have 0.613 g sample of a covalent compound contains 3.13 × 1021 molecules . We have to calculate…

Q: Sodium hydroxide reacts with carbon dioxide as follows: 2NaOH(s)+CO2(g)→Na2CO3(s)+H2O(l)   How…

A: Given, Chemical Reaction:  2NaOH(s)+CO2(g)→Na2CO3(s)+H2O(l) Moles of NaOH = 2.30 moles  NaOH is…

Q: How many moles of Feg04 are required to supply enough iron to prepare 0.843 mol Fe203? i mol Fe304

A:

Q: A flask contains 0.490 mol of liquid bromine, Br2Br2. Determine the number of bromine molecules…

A:

Q: Calculate the mass of hydrogen formed when 25 grams of aluminum reacts with excess hydrochloric…

A: Given: Mass of Aluminum = 25 g

Q: A sample of an oxide of vanadium weighing 4.589 g was reduced with hydrogen gas to form water and…

A: Solution :    The empirical formula gives the simple whole-number ratio of elements present in a…

Q: finding the number of moles of Zn(OH), produced i

A: To find the correct set up we need to correlate  Zn and Zn(OH)2 in terms of moles

Q: How many moles of H2 can be formed if a 2.78 g sample of Mg reacts with excess HC1?

A:

Q: A 19.91 g sample of Mo2O3(s) is converted completely to another molybdenum oxide by adding oxygen.…

A: Step 1:Identification of Emprical Formula of the New oxide.*n(Mo2O3) = m (Mo2O3)…

Q: N2(g) + 3 H,(g)→2 NH;(g) How many moles of NH, can be formed from 3.0 mol of N, and 6.0 mol of H,?

A: Given reaction is : N2 (g) + 3H2 (g) ---------> 2NH3 (g)  Moles of N2 = 3.0 mole  Moles of H2 =…

Q: Consider the following chemical reaction: 3Mg + B₂03 → 2B + 3 MgO. What mass in grams of magnesium…

A:

Q: An experiment requires that enough PNCl2 be used to yield 10.3 g of chlorine. How much PNCl2 must be…

A: Answer: 16.84 g

Q: A compound of mass 0.496g consisted of only C,H and O. It was completely burned in oxygen,producing…

A:

Q: 1.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have…

A:

Q: Use the following data and steps below to calculate the formula of the copper chloride hydrate.…

A: Since you have posted a question with multiple sub-parts , we will solve first three subparts for…

Q: cumene is compound comtaining only carbon and hydrogen that is used in the production of acetone and…

A: Interpretation: The range of molar mass of cumene that contains only carbon and hydrogen is given.…

Q: A student, Ken, is given a mixture containing two carbonate compounds. The mixture includes MgCO,…

A: Given: Percent by mass of CO32- ions in sample = 69.14 %

Q: What is the simplest or empirical formula of a compound which is found to have a mole ratio    of…

A: Given;

Q: An acid, HEI, is formed from a hypothetical element, El, and a subsequent aqueous solution is…

A: Percent by weight or %(w/w) :-  The mass of solute present in 100 grams of solution is defined as…

Q: What amount of carbon dioxide (in moles) is produced by the reaction of 5.00 mol C3H12 with 30.0 mol…

A:

Q: A piece of aluminum foil 1.00 cm square and 0.570 mm thick is allowed to react with bromine to form…

A: Using the given area and thickness, find the volume of aluminum foil.

Q: asolim and water (H,O). What mass of water is produced by the reaction of 7.74 g of octane?

A: The balanced equation for the combustion of octane is,                                    2 C8H18+25…

Q: A 2.20 g sample of an oxide of bromine is converted to 3.692 g of AgBr. Calculate the empirical…

A: Step : 1         Calculate the empirical formula of the oxide.

Q: Considering the limiting reactant concept, how many moles of copper sulfide are produced from the…

A:

Q: A sample of an oxide of vanadium weighing 4.589g was reduced with hydrogen gas to form water and…

A: The empirical formula represents the number of atoms in the molecule with the smallest positive…

Q: This reaction makes potassium superaxide useful in a self-contained breathing apparatus. How much Oz…

A: First calculate moles of KO2 and CO2. Then use mol to mol ratio to check which compound forms less…

Q: In one process, 5.75 kg of CaF, is treated with an excess of H,SO, and yields 2.45 kg of HF.…

A: Given :- mass of CaF2 = 5.75 kg  Actual yield of HF = 2.45 kg  To calculate :-  Percent yield of HF

Q: For the dehydration experiment, the mass of green crystals before heating was G.H g. After the…

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

Q: A 0.45g sample of aspirin is decomposed into its constituent elements and found to contain 0.27g C,…

A: Given: Mass of aspirin sample = 0.45 g. Mass of C produced = 0.27 g. Mass of H produced = 0.020 g…

Q: A chemist set up a synthesis of phosphorus trichloride (PCl3) by mixing 12.0 g of phosphorus (P)…

A: Given data: 12 g Phosphorous react with 35 g of chlorine to give 42.4 g of PCl3 . % yield of…

Q: Calculate the number of grams Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen

A: The reaction taking place will be  6 Li + N2 -----> 2 Li3N hence from the above reaction we can…

Q: A student used 1.50 g of manganese to react with excess fluorine to form manganese fluoride. If 4.09…

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.