A compound is found to contain 26.73 % phosphorus, 12.09 % nitrogen, and 61.18 % chlorine by weight. To answer the questions, enter the elements in the order presented above. 1. What is the empirical formula for this compound? 2. The molecular weight for this compound is 115.9 g/mol. What is the molecular formula for this compound?

Q: When 1.849 grams of a hydrocarbon, C,Hy, were burned in a combustion analysis apparatus, 6.249 grams…

A: Combustion reaction involves the reaction of the compound with oxygen. Combustion of hydrocarbon…

Q: Determine the molecular formula of a compound that contains 26.7% P, 12.1% N, and 61.2% Cl, and has…

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Q: A sample of sulfolane, C.H3O,S, contains 5.00 x 1024 atoms. How many moles of sulfolane are in the…

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Q: Complete the table. Element Moles Mass Cr 0.00442 Fe 73.5 mg Ti 1.009 x 10-3 Hg 1.78 kg

A: Mole is represented by the symbol mol. It is unit of measurement of substance. Mass is defined as…

Q: How can a molecular formula be obtained from an empirical formula? What additional information is…

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Q: A compound consisting of B, N, and H undergoes elemental analysis. The % composition by mass is…

A: Given,Percent of B in the compound = 40.28 %Percent of N in the compound = 52.20 %Percent of H in…

Q: An unknown compound contains only C, H, and O. Combustion of 6.30 g of this compound produced 12.6 g…

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Q: Complete combustion of 6.70 g of a hydrocarbon produced 20.7 g of CO₂ and 9.51 g of H₂O. What is the…

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Q: What is the difference between an empirical formula and a molecular formula? Provide an example.

A: There are three types of chemical formulas:-  Empirical formula is the simplest whole number of…

Q: Determine the chemical formula of a compound that contains 56.6% K, 8.69% C and 34.7% O. Write any…

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Q: 4. Determine the empirical formula of a compound with the following composition by mass: 48.0 % C,…

A: 4. Given, Molar mass of the compound = 200 g/mol Mass % of C = 48.0 % = 48.0 g Mass % of H = 8.0 % =…

Q: A compound is found to contain 31.42 % sulfur, 31.35 % oxygen, and 37.23 % fluorine by mass. What is…

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Q: When 4.510 grams of a hydrocarbon, CHy, wvere burned in a combustion analysis apparatus, 14.15 grams…

A: Whenever the combustion f a hydrocarbon takes place, only carbon dioxide and water vapors are…

Q: A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume a 100.-g sample of this compound. The…

A: Given, Mass % of C = 80.0 % Mass % of H = 20.0 % Mass of the compound = 100 g Empirical formula of…

Q: and 36.32% O by mass. What is its empirical formula? Insert subscripts as needed.   empirical…

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Q: 5. Determine the empirical and molecular formula of a compound whose composition is 85.7% C and…

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Q: 22. A 56.4 g sample of a compound with a molecular mass of 210 u was found to be composed of 12.35 g…

A: You have posted multiple questions, we can only solve first question for you according to the…

Q: 16) How many molecules of butane are contained in 25.0 mL of butane? The density of butane is 0.6011…

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Q: An unknown compound contains only C, H, and O. Combustion of 6.10 g of this compound produced 14.4 g…

A: Calculation of no. of mol of CO2: n=given massMolar mass=14.4 g44.01 g/mol=0.3272 mol 1 mol of CO2…

Q: Determine the empirical formula for a compound that contains C, H, and O. It contains 52.14% C, and…

A: % of H = 100-52.14-34.73= 13.13  Suppose we have 100 g sample . So moles of C =…

Q: The empirical formula and molar mass of several compounds are listed. Find the molecular formula of…

A: Molecular formula can be calculculated by using below formula : Molar massg/molEmpirical formula…

Q: Calculate the number of moles of carbon present in the following sample. 1.271 g of ethanol, C2H5OH

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Q: on, hydrogen and oxygen 180.16 g/mol.

A: a) moles of C = ( 3.66g / 44.0gmol-1 ) = 0.83mol .......(1)  Mass of C = ( moles of C ) • ( atomic…

Q: A certain compound is 52.2% carbon, 13.0% hydrogen, and 34.8% oxygen. Find the empirical formula of…

A: In order to find the empirical formula we first write down the given data: % of carbon= 52.2%. % of…

Q: The molar mass and empirical formula of several compounds listed. Find the molecular formula of…

A: Given: Empirical formula = C3H2N  Molar mass of compound = 312.29 g/mol Empirical formula mass = 52…

Q: Part D. A 28.50 g sample of a compound of carbon, sulfur, hydrogen, and combusted (burned). 35.25 g…

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Q: 13. Dichloroethane, a compound that is often used for dry cleaning, contains carbon, hydrogen, and…

A: When two or more atoms combine with each other, they will form molecule and those molecules has…

Q: An unknown compound contains only C , H , and O . Combustion of 6.90 g of this compound produced…

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Q: A 4.455 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis…

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Q: Determine molecular formula. An organic compound that only contains C, H, and O was subjected to…

A: Since the compound is made up of only C, H and O. Hence we can assume the empirical formula of…

Q: Determine if each formula below is empirical or molecular. Cas(PO4)2 CH4 NaCl

A: Following are the empirical and molecular formulas.

Q: osmium by mass. a) If you assume 100.0 g of the compound, what is the mass in grams of osmium that…

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

Q: When 1.440 g of a liquid hydrocarbon, CxHy, was burned in a combustion apparatus, 4.600 g of CO2 and…

A: The compound contains only Carbon and Hydrogen atoms. The number of moles of H2O and CO2 is…

Q: An unknown compound with a molar mass of 402.561 g/mol is made of 4.446 g of carbon, 1.741 g of…

A: To find the Molecule formula of given compund , first have to find the moles of carbon , Hydrogen…

Q: A compound has a molar mass of 38.41 g/mol.  If a sample of this compound is 246.1 g, how many mol…

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Q: An element analysis was performed on the liquid #1. It was discovered that it was 60.0% C, 13.3% H,…

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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.