10. A sample of a pure compound contains 12.23 g of nitrogen and 15.01 g of oxygen. The molar mass of this pure compound is about 90 g. Determine the empirical formula, the molecular formula, and the molar mass of this compound.

Q: empirical formula

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Q: What is the empirical formula mass of a compound?

A: The empirical formula of a compound identifies the elements contained in the compound as well as…

Q: A 0.858-g sample of copper was reacted with oxygen to form 1.074 g of copper oxide. Determine the…

A: Given, mass of copper sample = 0.858 g Mass of copper oxide formed = 1.074 g Empirical formula of…

Q: A 0.338-g sample of antimony was completely reacted with 0.295 g of chlorine gas to form antimony…

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Q: Measurements show that unknown compound X has the following composition: element mass % nitrogen…

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Q: Mass of crucible and cover is 43.92 g. The mass of crucible, cover, and magnesium is 44.62g. Mass of…

A: Empirical formula is the chemical formula  which represents the simple ratio of atoms of constituent…

Q: A compound has the empirical formula C3H2 and has a molar mass of 228.3 g/mol. What is the molecular…

A: The empirical formula of the compound is = C3H2 The molar mass of the compound is = 228.3 g/mol We…

Q: How can the Percentage Composition be obtained from chemical formulas?

A: Percentage composition is given by, % composition = mass of the elementTotal mass of the…

Q: A thimble of water contains 4.0 x 1021 molecules. The number of moles of H2O is:

A: Given: Number of molecules of water = 4.0×1021 molecules   We know that,    1 mole = 6.023×1023…

Q: What advantage is there to using a counting unit (the mole) for amount of substance rather than a…

A: To explain the advantage of using mole unit instead of mass unit.

Q: in a combustion analysis,0.0300 moles of element R reacts with 0.0350 moles of oxygen gas.Determine…

A: Given : moles of element R = 0.0300                                   moles of oxygen gas = 0.0350…

Q: Upon combustion, an unknown compound containing only carbon and hydrogen produces 60.48 g carbon…

A: As we know that in any combustion reaction mole is CO2 is equal to no of carbon in hydrocarbon while…

Q: 19. A sample of a compound contains 19.97g Ti and 13.37g O. Determine the empirical formula of the…

A: To find empirical formula, first we will calculate the moles of each element present in that…

Q: A compound containing only sulfur and nitrogen is 69.6% S by mass; the molar mass is 184 g/mol. What…

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Q: A compound that consists of nitrogen and oxygen is found to be 30.4 % nitrogen by mass. The molar…

A: Given : Nitrogen by mass = 30.4% Molar mass is in between 90g/mol and 100g/mol

Q: A compound is found to contain 37.47 % carbon, 12.61 % hydrogen, and 49.92 % oxygen by mass What is…

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Q: In a lab experiment it was  observed that 0.6884 g of lead combines with 0.2356 g chlorine to form…

A: Lead (Pb) combines with chlorine (Cl) and forms a binary compound. Mass of Pb=0.6884 g  Mass of…

Q: 22 A compound consists of 40.00% carbon, 6.71% hydrogen and 53.29% oxygen and has a molecular mass…

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Q: A 283.9 gram sample of an unknown compound was analyzed and found to consist of 17.54% sodium,…

A: Given :-  Percent composition by mass of Na = 17.54%  Percent composition by mass of Cr = 40.01%…

Q: A 9.478 gram sample of iron is heated in the presence of excess fluorine. A metal fluoride is formed…

A: The empirical formula represents the simplest whole number ratio of elements present in a compound.

Q: If a 25 g sample is composed of 9 g C and 16 g O, what is its empirical formula?

A: Given: mass of C = 9 g mass of O = 16 g molar mass of C = 12.0 g/mol molar mass of O = 16.0 g/mol

Q: A 20.97 gram sample of cobalt is heated in the presence of excess fluorine. A metal fluoride is…

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Q: a 9.37 g sample contains 0.731 g of carbon and 8.639 g of chlorine. determine the empirical formula…

A: To calculate the empirical formula of the compound, first it is required to calculate the number of…

Q: A new computer chip contains 4.71×1022 Si atoms. Determine the mass (in grams) of the silicon…

A: 1 mole of any substance contains avagadro number of atoms i.e.6.022×1023 atoms.  6.022×1023 atoms of…

Q: Determination of a chemical formula, mass of crucible is 14.9234g, crucible + hydrated  sample is…

A: Mass of hydrated sample =( Mass of crucible + hydrated sample) - Mass of crucible

Q: A compound is 22.76% Carbon, 68.30% Boron and 8.93% Hydrogen by mass. What is this compound’s…

A: The given percentage of different elements firstly changed into moles by deviding it by atomic…

Q: completely

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Q: A 0.77-mg sample of nitrogen reacts with chlorine to form 6.61 mg of the chloride. Determine the…

A: Mass of Nitrogen reacted = 0.77 mg Mass of Chlorine reacted = 6.61-0.77 =5.84 mg Dividing each of…

Q: A white powder is analyzed and found to contain 43.64% phosphorus, and 56.36% oxygen by mass. The…

A: Given: Percent by mass of P = 43.64 % Percent by mass of O = 56.36 % And molar mass of compound =…

Q: A sample of a pure compund contains 3.04g of nitrogen and 6.94 g of oxygen. The molar mass of this…

A: Since the compound is having only N and O  Hence assuming the compound to be having empirical…

Q: A white powder is analyzed and found to contain 43.64% phosphorus and 56.36% oxygen by mass.The…

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Q: 1.651 g of Silver is combined with 0.1224 g of oxygen. Find the empirical formula.

A: moles of silver combining = mass / atomic mass atomic mass of Ag = 108 g/mol Hence moles of Silver =…

Q: Measurements show that unknown compound X has the following composition: element mass % carbon 40.9%…

A: Consider the given information is as follows; Mass percent of carbon (C) = 40.9% Mass percent of…

Q: What is the empirical and molecular formulas

A: Given :-  Percent composition of N = 87.42 %  Percent composition of H = 12.58 %  Molar mass = 32.06…

Q: A sample of naphthalene was analyzed in the laboratory and it was determined that the sample…

A: Number of moles (mol) = Given mass (g)Molar mass (g/mol)Given that:Number of moles= 0.457 molesMolar…

Q: A compound with a molar mass of 60g/mol is 40.4% carbon, 6.7% hydrogen and 53.3% oxygen (by mass).…

A: An empirical formula is defined as the simplest or most reduced whole number ratio of atoms present…

Q: Determine the empirical formula for a compound that is composed of 40.60% carbon, 6.7% Hydrogen and…

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Q: Platinum forms two compounds with chlorine. One contains 26.7% Cl by mass and the other 42.1% Cl by…

A: In chemistry, the empirical formula of a chemical compound is the simplest whole number ratio of…

Q: A sample compound contains 19.97g Ti and 13.37g O. Determine the empirical formula of the compound.

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Q: mass of 1.2 × 10^23 atoms of phosphorus (molar mass= 31 gm/mo

A: The one mole of a substance contains 6.022×1023 number of its atoms.here moles of…

Q: On a weight basis, a compound is 39.1% car- bon, 52.2% oxygen and the rest is hydrogen. What is the…

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Q: A compound is found to contain 46.68% nitrogen and 53.32% oxygen by mass. What is the empirical…

A: Given, percentage of nitrogen =46.68% percentage of oxygen = 53.32 %

Q: Chemical analysis reveals that a sample of dioxin contains 14.29g of carbon, 1.20g of hydrogen, and…

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Q: Measurements show that unknown compound X has the following composition: element mass % carbon 62.1%…

A: Empirical formula is that formula of a chemical compound which gives the ratio or the proportions of…

Q: the empirical formula of a compound

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Q: A certain compound contains 10 carbon atoms, 18 hydrogen atoms, and 2 oxygen atoms. What is the…

A: MOLECULAR FORMULA  C10 H18 O2 EMPIRICAL FORMULA C5 H9 O ( C5 H9 O) X2 =C10 H18 O2

Q: A compound contains 12.8% C, 2.1% H, and 83.1% Br (by mass). Calculate the empirical formula and the…

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Q: C. A compound has been found to contain 38.8% K, 29.4% Mn by mass. The remainder of the compound is…

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Q: If 0.87g of nitrogen is combined with 6.61g of chlorine, find the empirical formula.

A: Given: Mass of nitrogen= 0.87 g Mass of chlorine= 6.61 g

Q: percent composition

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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.