Hydroxylammonium nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. What is its empirical formula?

Q: A certain mass of compound X (molar mass = 102.4) is dissolved in water to give 0.548 L of an 5.58…

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Q: Paracresol (p-cresol) is used as a disinfectant and in the manufacture of herbicides. A 0.4039 g…

A: Recall the data from the question Mass of sample=0.4039 g mass of carbon dioxide=1.1518 g mass of…

Q: A 2.68 gram sample of a KCl and KCIO3 mixture was found to contain 0.01541 mol of KCIO3. What is the…

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Q: Assuming one mole of compound, calculate the theoretical percentage composition of P₂O3. O P: 56.4%…

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Q: Morphine (C₁₇H₁₉NO₃) is a painkiller in the opiate family. A sample of morphine was discovered that…

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Q: How many grams of magnesium oxide can be produced by reacting 0.248 g magnesium that is 97.5% pure…

A: Given mass of Magnesium = 0.248g% purity of Magnesium = 97.5%No.of molecules of oxygen = 5.36 x…

Q: A particular compound is comprised only of the elements C, H, N, and Cl. Combustion analysis of…

A: Given that: Total mass of sample = 14.30 g Mass of CO2 = 31.22 g Mass of H2O = 6.764 g Mass % of N=…

Q: 5) 0.7971 g of molecule, X, is found to contain 3.0 x 1022 atoms. Deduce the identity of X. Given N…

A: Given: Mass of X2 = 0.7971 g Atoms of X2 = 3.0×1022 NA = 6.023×1023 mol-1

Q: C6H6 contaminates a water sample. The sample contains 0.000037% of the compound by mass. How much…

A: Mass percent = (Mass of solute/Mass of solution) x 100 Let us consider the mass percent of solution…

Q: A student weighs an empty beaker at 85.301 g. A sample of Na2SO4·??H2O is added to the beaker, and…

A: Mass of empty beaker = 85.301 g  Mass of beaker + hydrated salt = 86.607 g  Mass of beaker +…

Q: 1-Calculate the mass of compound required to prepare 100.00 mL of a 1.40x102 M CuCl2 ?.

A: Molarity is number of moles of solute present per liter of solution, notated as M and the unit is…

Q: When carbon-containing compounds are burned in a limited amount of air, some CO(g) as well as CO2(g)…

A: Mass percent of a compound is equal to the mass of component divided by total mass of the compound.

Q: A water solution of sulfuric acid (H2SO4) has a density of 1.864 g/mL and is 73.0% H2SO4 by mass.…

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Q: 011: calculate mass needed to prepare 5.0L of 0.10N Na,CO,(105.99g/mol) from standard solid.

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Q: A mixture was found to contain 1.50g NH4CI, 0.80 g NaCI, and 1.20 g SiO2. What is the percentage of…

A: Given: Mass of NH4Cl = 1.50 g Mass of NaCl = 0.80 g Mass of SiO2 = 1.20 g

Q: The aluminum in a 0.767 g sample of an unknown material was precipitated as aluminum hydroxide,…

A: given: mass of sample of unknown material =0.767 g mass of aluminium oxide produced = 0.143 g…

Q: Concentrated sulfuric acid (18.3 M) has a density of1.84 g/mL.(a) How many moles of H₂SO₄ are in…

A: The molecular mass of a substance is the sum of the atomic masses of all the atoms in a molecule of…

Q: Under certain conditions the reaction of N2 with excess H2 will produce a 72.09% yield of NH3. What…

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Q: What is the molecular formula of the molecule that has an empirical formula of CH and a molar mass…

A: Given , Empirical formula = CH Molar mass = 78.0 g/mol

Q: A 1.000 g sample of an unknown compound containing only carbon, hydrogen, and oxygen was analyzed…

A: Given: Mass of sample = 1.000 g Mass of CO2 formed = 2.579 g Mass of H₂O formed = 0.6536 g Molar…

Q: Methanol, which is present in mentholated cough drops, is an organic compound containing only C, H…

A: Combustion is a high-temperature exothermic redox chemical reaction between a fuel and an oxidant,…

Q: If 2.332 g of a sample containing a mixture of CuO and CuCO3 are heated, the final weight of the…

A: CuCO3 on heating decomposes to form CuO and CO2 CuCO3 (s) →heat CuO (s) + CO2 (g) 123.55 g…

Q: Compound X has a molar mass of 176.12·gmol−1 and the following composition: element mass % carbon…

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Q: A chemist weighs 50.0 grams of solid Mg(OH)2. How many moles of Mg(OH)2 are in the sample? How…

A: Given :-  Amount of Mg(OH)2 = 50.0 g  To Calculate :-  No.of moles of Mg(OH)2  No.of formula units…

Q: A sample containing only carbon,hydrogen,phosphorus and oxygen is subjected to elemental analysis.…

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Q: For the chemical reaction,   2NaOH+H2SO4⟶Na2SO4+2H2O2NaOH+H2SO4⟶Na2SO4+2H2O   what mass of…

A: The reaction is :  2 NaOH + H2SO4 ==> Na2SO4 + 2 H2O  Moles of water given = 4.87 mol  Molar mass…

Q: A 1.000 g sample of an unknown compound containing only carbon, hydrogen, and oxygen was analyzed…

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Q: Morphine (C₁₇H₁₉NO₃) is a painkiller in the opiate family. A sample of morphine was discovered that…

A: Given: When morphine undergoes combustion, carbon dioxide is produced. Mass of mixture            =…

Q: The density of octane, C8H18C8⁢H18, is 0.703 g/mL0.703 g/mL. Calculate the number of moles of octane…

A: Given Data :  1.density of octane = 0.703 g/mL  2. Volume = 49.1 mL  Molar mass of octane = 114.23…

Q: How many moles of Al are necessary to form 28.6 g of AlBr₃ from this reaction: 2 Al(s) + 3 Br₂(l) →…

A: Given , mass of AlBr₃  = 28.6 g Thus, moles of AlBr₃  = mass of AlBr₃ molar mass of AlBr₃  = 28.6…

Q: Suppose a student starts with 2.4319 g of a sand mixture and separates the components into 1.3012 g…

A: percent of SiO2 in the starting mixture =    =Mass of SiO2 × 100/ Total Mass of the mixture =…

Q: Calculate the mass percent of carbon in glucose (C6H12O6).

A: Dear student, since you have asked multiple questions but according to guidelines we will solve 1st…

Q: A compound contains C, H and O. If it contains 52.2% C and 34.7% O by mass, what is its empirical…

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Q: Calculate the mass percent of 0.389 g of silicon (Si) that reacts with oxygen to form 0.832 g…

A: Given that:  Si = 0.389g and SiO2 = 0.832 g…

Q: Determine the mass of a solution of a 7.897 wt % LiI if you needed to provide 0.3894 moles of LiI…

A: wt% = 100 x Mass of solute/Mass of solution Mass = Number of moles x molar mass

Q: . How many moles of Al(C 2 H 3 O 2 ) 3 contain 19mol O ? 6. Determine the % composition by mass of…

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Q: 1-Calculate the mass of compound required to prepare 100.00 mL of a 1.40x102 M CuCl2 ?.

A: Molecular weight of CuCl2 = 134.45 g mol-1 Formula Used 1. No of moles = volume × concentration 2.…

Q: Mass of NH4NO3 (s) + H2O (l) = 1.9871 Determine the moles of NH4NO3 in the sample. The molecular…

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Q: FORMULAS FROM PERCENT COMPOSITION: 8. %Zn = 11.44%; %U = 41.64; %C = 16.81%; %H = 2.12%; %O = 27.9

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Q: What is the percent NaCl in the sample?

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Q: 6. Calculate the stoichiometric formula of a compound, which is defined by the mass composition: C:…

A: The question is based on elemental chemistry. We need to calculate empirical formula of the given…

Q: What is the formula (solve for x) for the original hydrated sample of copper (II) sulphate? You…

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Q: Hydroxylammonium nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. What is its…

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Q: What volume of 1.772 M BaCl2 is needed to obtain 123 g of BaCl2?

A: BaCl2 = Barium Chloride Molecular weight of BaCl2  = Atomic wt of Ba + Cl x 2…

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.