16:49Introduction to Combustion Analysis, Empirical Formula & Molecular Formula ProblemsThe Organic Chemistry Tutor790views
02:52Finding and Calculating an Empirical Formula of a Compound | How to Pass ChemistryMelissa Maribel580views2rank
11:00Empirical Formula & Molecular Formula Determination From Percent CompositionThe Organic Chemistry Tutor642views
Multiple ChoiceWhich of the following could be both a molecular formula and an empirical formula?547views
Multiple ChoiceIn order to make 1 s’ more, you need 2 graham crackers, 1 piece of chocolate, and 1 marshmallow. How many s’mores can be made from the following ingredients? 7 graham crackers, 6 pieces of chocolate, and 5 marshmallows322views1rank
Multiple ChoiceA chemist wishing to identify a compound determines the masses of its elements as: 1.445 g S and 6.391 g Cl. Determine its empirical formula.235views
Multiple ChoiceDetermine the simplest form of a compound made up of carbon, hydrogen, nitrogen and oxygen if it is made of 49.48% C, 5.19% H and 16.48% O.236views
Multiple ChoiceA compound composed of potassium, manganese and oxygen contains 3.12 g potassium and 1.922 x 1023 oxygen atoms. If a sample of the compound weighs 12.61 g determine its empirical formula?241views5rank2comments
Textbook QuestionThe following diagram represents the collection of elements formed by a decomposition reaction. (b) Could you draw a diagram representing the molecules of the compound that had been decomposed? Why or why not?980views1rank
Textbook QuestionThe following diagram represents the collection of elements formed by a decomposition reaction. (a) If the blue spheres represent N atoms and the red ones represent O atoms, what was the empirical formula of the original compound?713views1rank
Textbook QuestionThe following diagram represents the collection of CO2 and H2O molecules formed by complete combustion of a hydrocarbon. What is the empirical formula of the hydrocarbon?794views1rank
Textbook QuestionDimethylhydrazine, a colorless liquid used as a rocket fuel, is 40.0% C, 13.3% H, and 46.7% N. What is the empirical formula? (LO 3.11) (a) CH4N9 (b) CH2N (c) C2H4N (d) C2H5N21024views
Textbook QuestionGive the empirical formula of each of the following compounds if a sample contains (c) 26.56% K, 35.41% Cr, and 38.03% O by mass.1431views
Textbook QuestionGive the empirical formula of each of the following compounds if a sample contains (b) 2.10 g nickel and 0.58 g oxygen459views
Textbook QuestionGive the empirical formula of each of the following compounds if a sample contains (a) 0.052 mol C, 0.103 mol H, and 0.017 mol O758views
Textbook QuestionThe structural formulas of the compounds n-butane and isobutane are shown below. (c) Which formulas—empirical, molecular, or structural—allow you determine these are different compounds?584views
Textbook QuestionThe structural formulas of the compounds n-butane and isobutane are shown below. (b) Determine the empirical formula of each.787views
Textbook QuestionDetermine the empirical formula of each of the following compounds if a sample contains (c) 89.14% Au and 10.86% O by mass.990views1rank
Textbook QuestionDetermine the empirical formula of each of the following compounds if a sample contains (b) 12.0 g calcium and 2.8 g nitrogen753views
Textbook QuestionDetermine the empirical formula of each of the following compounds if a sample contains (a) 3.92 mol C, 5.99 mol H, and 2.94 mol O637views
Textbook QuestionDetermine the empirical formulas of the compounds with the following compositions by mass: (b) 57.5% Na, 40.0% O, and 2.5% H709views
Textbook QuestionDetermine the empirical formulas of the compounds with the following compositions by mass: (a) 74.0% C, 8.7% H, and 17.3% N489views
Textbook QuestionWhat are the molecular and empirical formulas for each of the following compounds? Write the molecular formula for the following compound.510views
Textbook QuestionDetermine the empirical formulas of the compounds with the following compositions by mass: (c) 60.0% C, 4.4% H, and the remainder O525views
Textbook QuestionDetermine the empirical formulas of the compounds with the following compositions by mass: (a) 42.1% Na, 18.9% P, and 39.0% O1214views
Textbook QuestionTwo substances have the same molecular and empirical formulas. Does this mean that they must be the same compound?898views
Textbook QuestionWrite the empirical formula corresponding to each of the following molecular formulas: (e) C6H4Cl2645views
Textbook QuestionWrite the empirical formula corresponding to each of the following molecular formulas: (c) C4H8O2708views
Textbook QuestionWrite the empirical formula corresponding to each of the following molecular formulas: (b) C8H101000views
Textbook QuestionWrite the empirical formula corresponding to each of the following molecular formulas: (a) Al2Br6757views
Textbook QuestionDetermine the molecular and empirical formulas of the following: (b) the compound silicon tetrachloride, which has a silicon atom and four chlorine atoms and is used in the manufacture of computer chips1111views
Textbook QuestionDetermine the molecular and empirical formulas of the following: (a) the organic solvent benzene, which has six carbon atoms and six hydrogen atoms857views
Textbook QuestionSilver metal reacts with chlorine (Cl2) to yield silver chlo-ride. If 2.00 g of Ag reacts with 0.657 g of Cl2, what is the empirical formula of silver chloride?886views
Textbook QuestionWhat are the empirical formulas of substances with the following mass percent compositions? (c) Sodium thiosulfate (photographic 'fixer'): 30.36% O, 29.08% Na, 40.56% S777views
Textbook QuestionWhat are the empirical formulas of substances with the following mass percent compositions? (b) Ilmenite (a titanium-containing ore): 31.63% O, 31.56% Ti, 36.81% Fe753views
Textbook QuestionWhat are the empirical formulas of substances with the following mass percent compositions? (a) Aspirin: 4.48% H, 60.00% C, 35.52% O1640views
Textbook QuestionA chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. c. 2.128 g Be, 7.557 g S, 15.107 g O2081views2rank
Textbook QuestionA chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. b. 2.677 g Ba, 3.115 g Br463views
Textbook QuestionA chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. a. 1.245 g Ni, 5.381 g I675views
Textbook QuestionFerrocene, a substance proposed for use as a gasoline additive, has the percent composition 5.42% H, 64.56% C, and 30.02% Fe. What is the empirical formula of ferrocene?669views
Textbook QuestionCalculate the empirical formula for each stimulant based on its elemental mass percent composition. a. nicotine (found in tobacco leaves): C 74.03%, H 8.70%, N 17.27%1453views
Textbook QuestionCalculate the empirical formula for each natural flavor based on its elemental mass percent composition. b. vanillin (responsible for the taste and smell of vanilla): C 63.15%, H 5.30%, O 31.55%1028views
Textbook QuestionWhat is the empirical formula of stannous fluoride, the first fluoride compound added to toothpaste to protect teeth against decay? Its mass percent composition is 24.25% F, 75.75% Sn.635views
Textbook QuestionCalculate the empirical formula for each natural flavor based on its elemental mass percent composition. a. methyl butyrate (component of apple taste and smell): C 58.80%, H 9.87%, O 31.33%1204views
Textbook QuestionWhat are the empirical formulas of each of the following substances? (c) Zircon, a mineral from which cubic zirconia is made: 34.91% O, 15.32% Si, 49.77% Zr789views
Textbook QuestionWhat are the empirical formulas of each of the following substances? (b) Magnetite, a naturally occurring magnetic mineral: 72.36% Fe, 27.64% O718views
Textbook QuestionWhat are the empirical formulas of each of the following substances? (a) Ibuprofen, a headache remedy: 75.69% C, 15.51% O, 8.80% H637views
Textbook QuestionThe elemental mass percent composition of ibuprofen (a nonsteroidal anti-inflammatory drug [NSAID]) is 75.69% C, 8.80% H, and 15.51% O. Determine the empirical formula of ibuprofen.1461views
Textbook QuestionThe elemental mass percent composition of ascorbic acid (vitamin C) is 40.92% C, 4.58% H, and 54.50% O. Determine the empirical formula of ascorbic acid.2381views
Textbook QuestionA 45.2-mg sample of phosphorus reacts with selenium to form 131.6 mg of the selenide. Determine the empirical formula of phosphorus selenide.1881views1comments
Textbook QuestionCombustion analysis of a hydrocarbon produces 33.01 g CO2 and 13.51 g H2O. Calculate the empirical formula of the hydrocarbon.4664views
Textbook QuestionCombustion analysis of a 31.472 mg sample of the widely used flame retardant Decabrom gave 1.444 mg of CO2. Is the molecular formula of Decabrom C12Br10 or C12Br10O?518views
Textbook QuestionHeating elemental cesium and platinum together for two days at 973 K gives a dark red ionic compound that is 57.67% Cs and 42.33% Pt. (a) What is the empirical formula of the compound?430views
Textbook QuestionUnder special conditions, sulfur reacts with anhydrous liquid ammonia to form a binary compound of sulfur and nitrogen. The compound is found to consist of 69.6% S and 30.4% N. Measurements of its molecular mass yield a value of 184.3 g>mol. The compound occasionally detonates on being struck or when heated rapidly. The sulfur and nitrogen atoms of the molecule are joined in a ring. All the bonds in the ring are of the same length. (a) Calculate the empirical and molecular formulas for the substance.1247views
Textbook QuestionA copper wire having a mass of 2.196 g was allowed to react with an excess of sulfur. The excess sulfur was then burned, yielding SO2 gas. The mass of the copper sulfide produced was 2.748 g. (b) What is its empirical formula?538views
Textbook QuestionAn herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor expressed at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl. (c) What other information would you need to know about this compound to calculate its true molecular formula?662views
Textbook QuestionReaction of gaseous fluorine with compound X yields a sin- gle product Y, whose mass percent composition is 61.7% F and 38.3% Cl. (a) What is a probable molecular formula for product Y, and what is a probable formula for X?495views
Open QuestionWhat is the empirical formula of a compound that contains only iron and oxygen and is 22.27% oxygen?223views
Open QuestionIn general, what does a subscript (such as the "2" in H2) tell you about the molecule?191views
Open QuestionSome of the formulas below could be either molecular or empirical formulas; however, some could only be molecular formulas. Which of the following formulas must be molecular formulas? Select all that apply.177views
Open QuestionA 4.08 g sample of a compound of nitrogen and oxygen contains 3.01 g of oxygen. What is the empirical formula?184views
Open QuestionWhat is the empirical formula of a compound that contains 75% Ag and 25% Cl by mass?170views1rank
Open QuestionDetermine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.184views
Open QuestionWhat is the empirical formula of a compound that contains 85 Ag and 15 F by mass?156views
Open QuestionWhich pair consists of a molecular formula and its corresponding empirical formula?197views
Open QuestionWhat is the simplest whole-number ratio of atoms in a molecule or formula unit called?180views
Open QuestionDetermine the empirical formula for a compound that contains C, H and O. It contains 52.14% C and 34.73% O by mass.187views
Open QuestionWhat is the empirical formula for a compound if a sample contains 1.0 g of S and 1.5 g of O?173views
Open QuestionA molecule of a certain compound contains two nitrogen atoms and four oxygen atoms. What is the molecular formula for this compound?200views
Open QuestionA chemist decomposes samples of several compounds; the masses of their constituent elements are listed. calculate the empirical formula for each compound.260views
Open QuestionBased on the mole ratio you determined in part c, what is the empirical formula of this compound?469views
Open QuestionA sample of an iron-containing compound is 22.0% iron, 50.2% oxygen, and 27.8% chlorine by mass.334views
Open QuestionA molecule's molecular formula and its empirical formula always share the same chemical properties498views
Open QuestionDetermine the empirical formula for a compound that contains C, H and O. It contains 52.14% C and 34.73% O by mass.236views
Open QuestionDetermine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.234views
Open QuestionThe elemental mass percent composition of succinic acid is 40.68% C, 5.12% H, and 54.19% O.171views
Open QuestionWhat is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass?190views
Open QuestionA compound consists of 37.51 g C, 4.20 g H, and 58.29 g O. What is the empirical formula?163views
Open QuestionTo indicate the number of atoms of each element present in a molecular compound, scientists use -146views
Open QuestionWhat is the empirical formula for a compound if a sample contains 3.72 g of P and 21.28 g of Cl?156views
Open QuestionWhat is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?155views
Open QuestionWhich number indicates the number of atoms of each element in a molecule of a substance144views
Open QuestionThe elemental mass percent composition of malonic acid is 34.63% C, 3.87% H, and 61.50% O.141views
Open QuestionWhat is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?218views
Open QuestionUse subscripts to represent the number of each type of atom or ion in a molecule.128views
Open QuestionWhat is the empirical formula of a compound that contains 29% Na, 41% S, and 30% O by mass?176views
Open QuestionWhat is the empirical formula for a compound that is 43.6% phosphorus and 56.4% oxygen?161views