Which of the molecular formulas below is also an empirical formula?

Q: The mass of 5.15 moles of a compound is determined to be 298 g. What is the formula mass of the…

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Q: A compound with the empirical formula of CH2  was found to have a molar mass of approximately 84g.…

A: Given, A compound with the empirical formula of CH2  Molar mass of CH2 = 12+2= 14 gram/mol Having…

Q: What information must a chemist obtain in order todetermine the empirical formula of an…

A: An empirical formula is the simplest chemical formula of a compound that gives the proportions of…

Q: Consider the following four formulas: SO2, B2H6, CO, C4H2O2. Which of these formulas could be (a)…

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Q: What is the difference between an empirical formula and a molecular formula? Can they ever be the…

A: The empirical and the molecular formulas are both a type of chemical formulas. An empirical formula…

Q: From the following, pick those that are empirical forme

A: Simplest whole number ratio of constituent elements in a compound is called empirical formula…

Q: The empirical formula of a compound is CH. If themolar mass of this compound is about 78 g, what is…

A: Empirical formula is the simplest ratio of the elements in a compound whereas molecular formula is…

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: An organic compound was analyzed by mass spectrometry and found to contain 26.246% carbon, 3.671%…

A: The organic compound contains,  26.246% carbon, 3.671% hydrogen, and  [100-(26.246+3.671)] = 70.083%…

Q: Why do molecular, structural, and empirical formulas exist?

A: Why do molecular, structural, and empirical formulas exist?

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: A sample of chloroethane, C,H,CI, contains 0.274 mol of the compound. What is the mass of the…

A: Number of moles = mass ÷ molecular mass Mass of compound=  number of moles× molecular mass For…

Q: A compound is found to contain 58.80 % xenon, 7.166 % oxygen, and 34.04 % fluorine by mass. What is…

A: Given - % composition by mass of  following elements 58.80 % xenon 7.166 % oxygen 34.04 % fluorine…

Q: The molar mass of a compound is twice that of its empirical formula.How are the compound’s molecular…

A: The empirical formula of a compound gives the lowest whole number ratio of the elements present in a…

Q: Why is it important to use formulas (such as empirical, molecular, structural) in calculating…

A: Emperical formula(E.F.):- It shows the simplest number and types of atoms constituting the compound.…

Q: What is the formula of pyrite, and what is its molar mass?

A: S=Fe=S is the structure of pyrite.The formula for pyrite is FeS2

Q: A substance was found to contain 65.95% barium and 34.05% chlorine by mass upon analysis. What is…

A: Given that mass percent of barium is 65.95 % and mass percent of chlorine is 34.05%.

Q: What is the empirical formula for a compound composed of 0.0633 mol of carbon (C), 0.0211 mol of…

A: Given : Moles of C = 0.0633 mol  Moles of H = 0.0211 mol  Moles of N = 0.0422 mol

Q: A compound of iron and oxygen is found to contain 69.94% iron and 30.06% oxygen. What will be the…

A: An empirical formula tells the smallest whole-number ratio of atoms present in a compound. To…

Q: An oxide of iron is 77.73% iron by mass; the rest is oxygen. Enter the empirical formula of this…

A: Given :-  Percent composition of Fe = 77.73 %  Percent composition of O = (100-77.73)%…

Q: Compound X is consisting of 38.70% carbon, 51.60% oxygen and the rest is hydrogen. The molar mass of…

A: Given:  Mass ℅ of carbon = 38.70 ℅ Mass ℅ of oxygen = 51.60 ℅

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

A: Write the empirical formula of X....

Q: Writing Empirical Formulas from Chemical Formulas

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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: A compound is found to contain 64.80 % carbon, 13.62 % hydrogen, and 21.58 % oxygen by mass. What is…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: What is the difference between empirical formula and molecular formula

A: Empirical formula of a chemical compound is the simplest positive integer ratio of atoms present in…

Q: A compound is found to contain 29.68 % sulfur and 70.32 % fluorine by mass. What is the empirical…

A: The simplest formula represents the smallest ratio of atoms present in a compound is known as…

Q: If an oxide of magnesium is 40% oxygen by mass, what is its empirical formula?

A: here, we have to calculate the empherical formula of oxide of Magnesium. we know the molar masses,…

Q: What is the empirical formula for this compound?

A: Number of moles = mass/molar mass  Molar mass of Oxygen = 16 g/mol  Molar mass of nitrogen = 14…

Q: empirical formula?

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Q: what are the molecular weights (molar mass) of the following compounds

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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: There is a series of nitrogen oxides that have the general formula NxOy.  What is the empirical…

A: Given :-  General formula of nitrogen oxide = NxOy  Percent composition by mass of N = 25.94%  To…

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

A: Given;

Q: A compound is found to contain 39.10% carbon, 7.67% hydrogen, 26.11% oxygen, 16.82% phoshorus, and…

A: Given,

Q: The characteristic odor of decaying flesh is due to the presence of various nitrogen-containing…

A: The molar mass of any substance is the mass present in one mole of the substance and the molecular…

Q: 0.374g of phosphorous was reacted with chlorine, the resulting mass was 2.515g. What is the…

A: Given that -  Mass of phosphorus = 0.374 g  Mass of produced Phosphorus Chloride = 2.515 g  Then,…

Q: What are the molecular weights (molar mass) of the following compounds

A: We need to determine the molar mass of MgCl2 and (NH4)2SO4.

Q: An organic acid contains 40.92% C, 54.50 % O, 4.58 % H, by mass. The molecular mass is 176 g/mole.…

A: We have given that  Molar mass = 176g/mole  Percent composition of C = 40.92%  Percent composition…

Q: Which one of the following contains the most moles of hydrogen atoms?

A: (A) Each C2H6 contains 6 H atoms.  5 mol of C2H6 contains 6 x 5 = 30 mol of H atoms.

Q: What is the empirical formula for copper gluconate

A: In this question, we will write the empirical formula for copper gluconate.  You can see details…

Q: The percent by mass of nitrogen for a compound is found to be 30.5%, Which of the following could be…

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Q: If an oxide of magnesium is 50% oxygen by mass, what is its empirical formula?

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Q: A compound is found to contain 7.522% phosphorus and 92.47 % iodine  by mass. a. What is the…

A: From the mole ratio of the element we can determine the empirical formula . Using empirical formula…

Q: A compound is composed of 27.29% C and 72.71% O by mass. What is its empirical formula?

A: The empirical formula shows the kind and proportions of atoms in a substance in its simplest form.…

Q: A substance has the molecular formula C3HO6. What is its empirical formula?

A: We need to find the empirical formula for given compound

Q: A sample of dichlorodiiodosilane, SiCl,I,, contains 0.0462 mol of the compound. What is the mass of…

A: Given that: Moles of SiCl2I2 = 0.0462 moles Mass of SiCl2I2 = ?

Q: Elemental analysis of a compound produced the following results: 93.711% carbon and 6.289% hydrogen.…

A: Given that : A compound is produced by 93.711% carbon and 6.289% hydrogen. We have to determine 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.