A compound has the composition of 54.53% Carbon, 9.15% Hydrogen, and 36.32% Oxygen, by mass. If the molar mass is 88.1 g/mol, what is its molecular formula?            (A) C2H4O                                 (B) C4H8O2                                (C) C6H10O2                               (D) C6H12O3

Q: How many atoms or ions of each element are in 157.3 g of the following substances? (a) H₂ x 1025 H…

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Q: The molar masses and empirical formulas of several compounds containing carbon and nitrogen are…

A: The relatively simple positive integer ratio of all atoms contained in a chemical compound is…

Q: Calculate (to the nearest 0.1 u) the formula mass of these compounds. (a) boron trifluoride, BF3…

A: The compounds given are BF3, SrSO4 and CCl4.

Q: 1. Use chemical symbols to generate the factor needed to convert the weight of the substance in uie…

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

Q: 2. If the mass of H4X3 is 40 g, then X must represe (1) O (2) CI (3) Kr (4) C

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Q: The molecular formula for caffeine, one of the key compounds found in coffee and tea, is C8H10N4O2.…

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Q: (a) cyclobutane,     Molar Mass = (b) cobalt(III) chromate, Co2(CrO4)3   Molar Mass =

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Q: A binary compound of oxygen and an unknown element, x, has the formu XO and is 39.70 mass % oxygen.…

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Q: (2)lf 1.775 g of arsenic react with selenium to give 4.583 g of arsenic selenide, what is the…

A: we have to calculate the empirical formula of the compound

Q: Ethyl alcohol (C₂H5OH), also called grain alcohol, can be made by the fermentation of glucose:…

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Q: 1

A: Moles of propane = ( molecules of Propane / avagadro number )  Moles of propane = ( 3.45 • 10^24 /…

Q: Compound Y contains lead and oxygen only. 15.0 g of Y was found to contain 12.99 g lead. Find out…

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Q: Calculate the molar mass of each of the following:(a) S8(b) C5H12(c) Sc2(SO4)3(d) CH3COCH3…

A: (a) (b)

Q: ii) Calculate the percentage of carbon present in CeH12O6 (Atomic Mass of C-12 g, 0-16g and H-1g)

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Q: Determine the empirical formula of each of the following compounds. (Type your answer using the…

A: Data given:  (a) Number of moles of chlorine = 0.063 mol Number of moles of oxygen = 0.22 (b) Mass…

Q: 9. Which of the following has the greatest number of particles? (A) 9.012 g of Be (B) 1 mole of Na…

A: The no of moles is the ratio of given mass to that of molar mass of that substance.  For more than…

Q: Acetaminophen, an analgesic and antipyreticdrug, has a molecular mass of 151.2 u and a masspercent…

A: Given that:                  Molecular mass of acetaminophen = 151.2 u…

Q: Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced…

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Q: How many grams of Cl are in 38.0 g of each sample of chlo-rofluorocarbons (CFCs)? (a) CF2Cl2(b)…

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Q: A compound has the composition of 26.28% Carbon, 5.15% Hydrogen, 10.22% Nitrogen, and 58.35% Oxygen,…

A: Since percent composition is given, let's consider 100 g of the compound. For 100 g of the compound,…

Q: (3) Calculate the formula weight of the following compounds from their formulas Ca3(PO4)2 , CSH1206…

A: The formula weight of an ionic compound is sum of atomic masses of individual atoms present in the…

Q: Uranium is used as a fuel, primarily in the form of uranium(IV) oxide, in nuclear power plants. A…

A: To solve this problem first we have to calculate the mass of oxygen combined , then we will…

Q: (a) How many moles of ammonium ions are in 0.642 g of ammonium carbonate? 8.04e21 X mol (b) What is…

A: We have to calculate the required quantities.

Q: A 3.06 mg sample of a compound containing carbon, hydrogen, and oxygen underwent combustion…

A: “Since you have posted multiple questions, we will provide the  solution   only to the first…

Q: A 2.78 mg sample of a compound containing carbon, hydrogen, and oxygen underwent combustion…

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

Q: If you have 10.51 grams of palladium (IV) nitrate, how many moles is this? (b) If you have 7.12…

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Q: Q5) Determine the empirical formula of a compound that has (by mass) 85.7% carbon, 14.28% budr

A: We know that No of moles = mass / molar mass   For carbon - - > Moles of carbon = 85.7 g /…

Q: Give the empirical formula of each of the following compounds if a sample contains the following…

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Q: compound has the composition of 66.6% Carbon, 11.2% Hydrogen, and 22.2% Oxygen, by mass. If the…

A: Given is, 66.6% Carbon, 11.2% Hydrogen, and 22.2% Oxygen Molar mass= 144.2 g/mol

Q: What is the mass of 3.01 × 1023 molecules of nitrogen, N2? (A) 7.00 g (B) 14.0 g (C) 28.0 g (D) 42.0…

A: Number of molecules of N2 = 3.01 × 1023 One mole contains Avogadro’s number of atoms. Therefore,…

Q: In the case of incomplete combustion, the mass of carbon in the compound is the sum of carbons in…

A: Given, A Compound contains, Carbon, hydrogen and nitrogen mass of the compound = 0.1156 g Mass of…

Q: Calculate each of the following quantities:(a) Total number of ions in 38.1 g of SrF₂(b) Mass in…

A: The number of moles is equal to the ratio of mass to the molar mass of the substance. The total…

Q: Calculate the following: (a) mass in 1.73 mol of CaH 2 (b) moles of mg (NO3) 2 in 3.25 g of…

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Q: (a) What is the mass, in grams, of 4.62  1023 molecules of aspirin, C9H8O4?

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Q: How many iters of CH.OH gas are formed when 3.20 Lof H: gas are completely reacted at STP according…

A: using the given equation:-  CO + 2H2 → CH3OH Moles=given volume (L)22.4L2  mole of H2 produce 1 mole…

Q: Which of the following is a molecular compound?

A: a) Nacl -sodium chloride ionic  Na+/Cl-  b) NaoH -sodium hydroxide ionic Na+ /OH -  C)Fe PO4-  Iron…

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

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Q: a) Using NO2(g) as an example, show with dimensional analysis that the molecular mass and molar mass…

A: To convert u (amu) to g/mol, u is converted to g and then multiplied with the Avogadro constant.…

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.