16:49Introduction to Combustion Analysis, Empirical Formula & Molecular Formula ProblemsThe Organic Chemistry Tutor800views
02:52Finding and Calculating an Empirical Formula of a Compound | How to Pass ChemistryMelissa Maribel586views2rank
11:00Empirical Formula & Molecular Formula Determination From Percent CompositionThe Organic Chemistry Tutor649views
Multiple ChoiceWhich of the following could be both a molecular formula and an empirical formula?551views
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 marshmallows327views1rank
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.246views
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.244views
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?252views6rank2comments
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?997views1rank
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?721views1rank
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?806views1rank
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) C2H5N21034views
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.1438views
Textbook QuestionGive the empirical formula of each of the following compounds if a sample contains (b) 2.10 g nickel and 0.58 g oxygen467views
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 O769views
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?594views
Textbook QuestionThe structural formulas of the compounds n-butane and isobutane are shown below. (b) Determine the empirical formula of each.800views
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.1001views1rank
Textbook QuestionDetermine the empirical formula of each of the following compounds if a sample contains (b) 12.0 g calcium and 2.8 g nitrogen760views
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 O642views
Textbook QuestionDetermine the empirical formulas of the compounds with the following compositions by mass: (b) 57.5% Na, 40.0% O, and 2.5% H713views
Textbook QuestionDetermine the empirical formulas of the compounds with the following compositions by mass: (a) 74.0% C, 8.7% H, and 17.3% N493views
Textbook QuestionWhat are the molecular and empirical formulas for each of the following compounds? Write the molecular formula for the following compound.519views
Textbook QuestionDetermine the empirical formulas of the compounds with the following compositions by mass: (c) 60.0% C, 4.4% H, and the remainder O530views
Textbook QuestionDetermine the empirical formulas of the compounds with the following compositions by mass: (a) 42.1% Na, 18.9% P, and 39.0% O1230views
Textbook QuestionTwo substances have the same molecular and empirical formulas. Does this mean that they must be the same compound?906views
Textbook QuestionWrite the empirical formula corresponding to each of the following molecular formulas: (e) C6H4Cl2651views
Textbook QuestionWrite the empirical formula corresponding to each of the following molecular formulas: (c) C4H8O2713views
Textbook QuestionWrite the empirical formula corresponding to each of the following molecular formulas: (b) C8H101008views
Textbook QuestionWrite the empirical formula corresponding to each of the following molecular formulas: (a) Al2Br6767views
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 chips1119views
Textbook QuestionDetermine the molecular and empirical formulas of the following: (a) the organic solvent benzene, which has six carbon atoms and six hydrogen atoms863views
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?895views
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% S783views
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% Fe756views
Textbook QuestionWhat are the empirical formulas of substances with the following mass percent compositions? (a) Aspirin: 4.48% H, 60.00% C, 35.52% O1658views
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 O2107views2rank
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 Br464views
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 I681views
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?676views
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%1465views
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%1037views
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.643views
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%1215views
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% Zr795views
Textbook QuestionWhat are the empirical formulas of each of the following substances? (b) Magnetite, a naturally occurring magnetic mineral: 72.36% Fe, 27.64% O727views
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% H640views
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.1475views
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.2403views
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.1918views1comments
Textbook QuestionCombustion analysis of a hydrocarbon produces 33.01 g CO2 and 13.51 g H2O. Calculate the empirical formula of the hydrocarbon.4696views
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?525views
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?434views
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.1269views
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?542views
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?667views
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?498views
Open QuestionWhat is the empirical formula of a compound that contains only iron and oxygen and is 22.27% oxygen?231views
Open QuestionIn general, what does a subscript (such as the "2" in H2) tell you about the molecule?199views
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.183views
Open QuestionA 4.08 g sample of a compound of nitrogen and oxygen contains 3.01 g of oxygen. What is the empirical formula?188views
Open QuestionWhat is the empirical formula of a compound that contains 75% Ag and 25% Cl by mass?173views1rank
Open QuestionDetermine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.189views
Open QuestionWhat is the empirical formula of a compound that contains 85 Ag and 15 F by mass?160views
Open QuestionWhich pair consists of a molecular formula and its corresponding empirical formula?200views
Open QuestionWhat is the simplest whole-number ratio of atoms in a molecule or formula unit called?185views
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.193views
Open QuestionWhat is the empirical formula for a compound if a sample contains 1.0 g of S and 1.5 g of O?175views
Open QuestionA molecule of a certain compound contains two nitrogen atoms and four oxygen atoms. What is the molecular formula for this compound?203views
Open QuestionA chemist decomposes samples of several compounds; the masses of their constituent elements are listed. calculate the empirical formula for each compound.266views
Open QuestionBased on the mole ratio you determined in part c, what is the empirical formula of this compound?473views
Open QuestionA sample of an iron-containing compound is 22.0% iron, 50.2% oxygen, and 27.8% chlorine by mass.338views
Open QuestionA molecule's molecular formula and its empirical formula always share the same chemical properties507views
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.240views
Open QuestionDetermine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.237views
Open QuestionThe elemental mass percent composition of succinic acid is 40.68% C, 5.12% H, and 54.19% O.178views
Open QuestionWhat is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass?192views
Open QuestionA compound consists of 37.51 g C, 4.20 g H, and 58.29 g O. What is the empirical formula?166views
Open QuestionTo indicate the number of atoms of each element present in a molecular compound, scientists use -148views
Open QuestionWhat is the empirical formula for a compound if a sample contains 3.72 g of P and 21.28 g of Cl?159views
Open QuestionWhat is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?158views
Open QuestionWhich number indicates the number of atoms of each element in a molecule of a substance148views
Open QuestionThe elemental mass percent composition of malonic acid is 34.63% C, 3.87% H, and 61.50% O.144views
Open QuestionWhat is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?230views
Open QuestionUse subscripts to represent the number of each type of atom or ion in a molecule.131views
Open QuestionWhat is the empirical formula of a compound that contains 29% Na, 41% S, and 30% O by mass?183views
Open QuestionWhat is the empirical formula for a compound that is 43.6% phosphorus and 56.4% oxygen?164views