compound has the mass percent data given below . Determine its empirical formula. 32.43 % carbon by mass 8.16 \% hydrogen by mass 21.60 % oxygen by mass 37.81 % nitrogen by mass

Q: What is the mass in grams of 0.375 mole diatomic chlorine?     13.3 g     0.0134 g     2.26 x…

A: Moles of component is defined as ratio of the given mass to the molar mass. The relation for the…

Q: Commercial aqueous nitric acid is 71% HNO3 by mass and 16 M. Determine the density of this aqueous…

A: The percentage by mass of nitric acid solution = 71% Molarity of HNO3 = 16 M To calculate:…

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Q: 1. A certain compound is accidentally synthesized by a chemist in a laboratory set-up. He discovers…

A: Number of moles of any substance = mass of substance/molar mass of substance  Mol ratio for…

Q: Compound X2Z contains 32.2% X by mass. What mass of the compound contains 36.7 g X?

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Q: Show all the steps to determine the empirical formula for a compound with a percentage composition…

A: In a compound, the percent of each element that exists in terms of mass value is termed as its mass…

Q: A compound is analyzed and found to contain 12.1% carbon, 16.2% oxygen, and 71.7% chlorine (by…

A: Assuming 100 g of the compoun. Given : % of C = 12.1 %  % of O = 16.2 %  % of Cl = 71.7 %

Q: To determine the amount of platinum in an alloy, a 8.565 g8.565 g sample of an alloy containing…

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Q: Calculate the empirical formula for a compound that is 60.87% C, 4.38% H, and 34.75% O by mass…

A: C : 60.87% H : 4.38%  O : 34.75%

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A: Given: chemical formula of the talc. To find : Total number of moles of oxygen in the sample.…

Q: A crucible is placed on a balance and is found to have a mass of 26.639 grams a sample of…

A: Mass of crucible = 26.639 g Mass of crucible + mass of Na2SO4·xH2O = 27.085 g Therefore mass of…

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Q: The chemical formula for octane is: CH;(CH,),CH, Calculate the molar mass of octane. Round your…

A: To calculate the molar mass of octane.

Q: An organic compound consists of carbon, hydrogen and sulfur only. The percentage of carbon by mass…

A: For calculation of Molecular formula, first of all we calculate the % of each atom , empirical…

Q: What mass in grams of the magnetic oxide of iron (Fe3O4) can be made from 77.0 g of pure iron and an…

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Q: Nitrogen and oxygen form an extensive series of oxides with the general formula NxOy. What is the…

A: Given:  Empirical formula of Nitrogen oxide is NxOy.

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A: Since on heating the compound, the mass of water will be lost as it will get vaporised  Hence the…

Q: The analysis of a compound gives the following percent composition by mass: C: 56.70 percent; H:…

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Q: compound is 92.2% Carbon and 7.76% Hydrogen. The formula mass of the compound is 78.1 g. Calculate…

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Q: Question attached

A: Molarity is defined as “the mole of the solute per unit volume of the solution”. It is represented…

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A: Given that -  Percentage purity of urea , CH4N2O is = 55%  Molar/atomic masses are -  C = 12.01…

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Q: a. Determine the empirical formula for a compound with mass percent 48.91% Carbon, 18.51%…

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A: It is given that, The empirical formula of compound  is  C5H8O2 Molar mass = 300 g/mol So, we can…

Q: What is the mass percentage of carbon in C7H11O3? Express your answer as a percentage (i.e., out of…

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Q: Determine the mass in milligrams of 0.857 mol NH, CI. mg NH,Cl mass: Determine the mass in…

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Q: explain why the number of atoms and moles are different when the volumes are nearly identical?

A: 1. The table contains the data required to solve this problem.

Q: You analyze a sample of a compound you made in the lab and find that it has a percent composition by…

A: Answer: Empirical formula is C4H2O and three answers from the  given list are C4, H2, and O.

Q: the mass percentage composition of the elements in caffeine, C8H10N4O2.

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Q: B. TRUE OR FALSE: Read each statement carefully. Write TRUE if the statement is correct and FALSE if…

A: Percentage composition gives a brief ideas about each elemental composition as follows.

Q: Use the molar mass of Ca3(PO3)2 to calculate the number of formula units in 10.0 g of CP.  Give your…

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Q: Using your knowledge of molar mass and calculation, calculate the molar mass of the hypothetic…

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Q: A gaseous compound containing carbon and hydrogen was analyzed and found to consist of 83.65% carbon…

A: Suppose Total mass   = 100 gram  Mass of Carbon         = 83.65 gram Mass of Hydrogen     =…

Q: A. Determine the empirical formula for a compound with mass percent 48.91% carbon 18.51% hydrogen…

A: Suppose total mass of the compound as 100 g.          Mass of C=48.91 gMass of H=18.51 gMass of…

Q: Calculate the molar mass of chromium(III) chloride hexahydrate, CrCl3•6H2O, to 4 significant…

A: molar mass of chromium(III) chloride hexahydrate, CrCl3•6H2O is B

Q: 35. Calculate the mass in grams of each of the following samples. a. 1.25 moles of aluminum chloride…

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Q: Why should a pure compound have a definite composition by weight? how is it possible for two samples…

A: We need to explain why a pure compound is expected to have a definite composition.  Definite…

Q: Calculating Percent Composition Directions Use the equation below to calculate the percent…

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Q: The mineral iron pyrite (FeS2), typically, has a mass percentage of what is known as fool’s gold of…

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Q: 01.)What is the molecular formula of a compound with the empirical formula As2O5and a formula mass…

A: Given values are,  Empirical formula= As2O5 And formula mass = molar mass= 459.678 amu Now from…

Q: How do I do this problem? Determine the empirical formula of a compound having the following…

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Q: 1.The compuond cisplatin Pt(NH3)2Cl2 is an antitumor. a)Calculate the elemental percent composition…

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Q: In an experiment to determine the empirical formula of Tin Oxide, the following data were collected…

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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.