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chemistry a molecular approach
Chemistry A Molecular Approach 5th Edition Nivaldo Tro - Solutions
Determine the number of each type of atom in each formula.a. Mg3(PO4)2b. BaCl2c. Fe(NO2)2d. Ca(OH)2
Determine the number of each type of atom in each formula.a. Ca(NO2)2b. CuSO4c. Al(NO3)3d. Mg(HCO3)2
Write a chemical formula for each molecular model. a. b.
Classify each element as atomic or molecular.a. Neonb. Fluorinec. Potassiumd. Nitrogen
Identify the elements that have molecules as their basic units.a. Hydrogenb. Iodinec. Leadd. Oxygen
Butanedione—the component responsible for the smell and taste of butter and cheese—contains the elements carbon, hydrogen, and oxygen. The empirical formula of butanedione is C2H3O, and its molar mass is 86.09 g/mol. Determine its molecular formula. SORT You are given the empirical formula
What is combustion analysis? What is it used for?
A laboratory analysis of aspirin determines the following mass percent composition:C 60.00%; H 4.48%; O 35.52%Find the empirical formula. GIVEN: In a 100-g sample: 60.00 g C, 4.48 g H, 35.52 g O FIND: empirical formula
How can a molecular formula be obtained from an empirical formula? What additional information is required?
A compound containing nitrogen and oxygen is decomposed in the laboratory.It produces 24.5 g nitrogen and 70.0 g oxygen. Calculate the empirical formula of the compound. GIVEN: 24.5 g N, 70.0 g O FIND: empirical formula
Hydrogen may be used in the future to replace gasoline as a fuel. Most major automobile companies are developing vehicles that run on hydrogen. These cars have the potential to be less environmentally harmful than our current vehicles because their only emission is water vapor. One way to obtain
What kind of chemical formula can be obtained from experimental data showing the relative masses of the elements in a compound?
What kinds of conversion factors are inherent in chemical formulas? Provide an example.
The U.S. Food and Drug Administration (FDA) recommends that an adult consume less than 2.4 g of sodium per day. What mass of sodium chloride (in grams) can you consume and still be within the FDA guidelines?Sodium chloride is 39% sodium by mass. SORT You are given a mass of sodium and the mass
Calculate the mass percent of Cl in Freon-112 (C2Cl4F2), a CFC refrigerant. SORT You are given the molecular formula of Freon-112 and asked to find the mass percent of Cl. STRATEGIZE The molecular formula tells you that there are 4 mol of Cl in each mole of Freon-112. Find the mass percent
Explain how you can use the information in a chemical formula to determine how much of a particular element is present in a given amount of a compound. Provide some examples of why this might be important.
A compound has the empirical formula CH2O and a formula mass of 120.10 amu. What is the molecular formula of the compound?a) CH2Ob) C2H4O2c) C3H6O3d) C4H8O4
An aspirin tablet contains 325 mg of acetylsalicylic acid (C9H8O4). How many acetylsalicylic acid molecules does it contain? SORT You are given the mass of acetylsali- cylic acid and asked to find the number of molecules. STRATEGIZE First convert to moles (using the molar mass of the compound) and
What is the formula mass for a compound? Why is it useful?
A compound is 52.14% C, 13.13% H, and 34.73% O by mass.What is the empirical formula of the compound?a) C2H8O3b) C2H6Oc) C4HO3d) C3HO6
Based on the molecular views, classify each substance as an atomic element, a molecular element, an ionic compound, or a molecular compound. a. C. b.
Classify each compound as ionic or molecular.a. CO2b. NiCl2c. NaId. PCl3
Classify each compound as ionic or molecular.a. CF2Cl2b. CCl4c. PtO2d. SO3
Based on the molecular views, classify each substance as an atomic element, a molecular element, an ionic compound, or a molecular compound. a. C. b.
Write a formula for the ionic compound that forms between each pair of elements.a. Calcium and oxygenb. Zinc and sulfurc. Rubidium and bromined. Aluminum and oxygen
Write a formula for the ionic compound that forms between each pair of elements.a. Silver and chlorine b. Sodium and sulfur c. Aluminum and sulfur d. Potassium and chlorine
Write a formula for the compound that forms between calcium and each polyatomic ion.a. Hydroxideb. Chromatec. Phosphated. Cyanide
Write a formula for the compound that forms between potassium and each polyatomic ion.a. Carbonateb. Phosphatec. Hydrogen phosphated. Acetate
Name each ionic compound.a. Mg3N2b. KF c. Na2Od. Li2S e. CsF f. KI
Name each ionic compound.a. SnCl4 b. PbI2 c. Fe2O3d. CuI2 e. HgBr2 f. CrCl2
Give each ionic compound an appropriate name.a. SnO b. Cr2S3 c. RbI d. BaBr2
Give each ionic compound an appropriate name.a. BaS b. FeCl3 c. PbI4 d. SrBr2
Name each ionic compound containing a polyatomic ion.a. CuNO2 b. Mg(C2H3O2)2c. Ba(NO3)2 d. Pb(C2H3O2)2
Name each ionic compound containing a polyatomic ion.a. Ba(OH)2 b. NH4I c. NaBrO4d. Fe(OH)3
Write the formula for each ionic compound.a. Sodium hydrogen sulfiteb. Lithium permanganatec. Silver nitrated. Potassium sulfatee. Rubidium hydrogen sulfatef. Potassium hydrogen carbonate
Write the name from the formula or the formula from the name for each hydrated ionic compound.a. CoSO4 · 7 H2Ob. Iridium(III) bromide tetrahydratec. Mg(BrO3)2 · 6 H2Od. Potassium carbonate dihydrate
Write the formula for each ionic compound.a. Copper(II) chlorideb. Copper(I) iodatec. Lead(II) chromated. Calcium fluoridee. Potassium hydroxidef. Iron(II) phosphate
Name each molecular compound.a. CO b. NI3 c. SiCl4d. N4Se4
Write the name from the formula or the formula from the name for each hydrated ionic compound.a. Cobalt(II) phosphate octahydrateb. BeCl2 · 2 H2Oc. Chromium(III) phosphate trihydrated. LiNO2 · H2O
Name each molecular compound.a. SO3 b. SO2 c. BrF5 d. NO
Write the formula for each molecular compound.a. Phosphorus trichlorideb. Chlorine monoxidec. Disulfur tetrafluorided. Phosphorus pentafluoride
Write the formula for each molecular compound.a. Boron tribromideb. Dichlorine monoxidec. Xenon tetrafluorided. Carbon tetrabromide
Name each acid.a. HI(aq)b. HNO3(aq)c. H2CO3(aq)
Name each acid.a. HCl(aq) b. HClO2(aq) c. H2SO4(aq)
Refer to the nomenclature flowchart (Figure 3.11) to name each compound.a. SrCl2 b. SnO2c. P2S5 d. HC2H3O2(aq) Inorganic Nomenclature Flowchart IONIC Metal and nonmetal Metal forms one type of ion only. name of base name of cation anion (nonmetal) (metal) + -ide Example: Cal₂ calcium
Write the formula for each acid.a. Hydrofluoric acidb. Hydrobromic acidc. Sulfurous acid
Refer to the nomenclature flowchart (Figure 3.11) to name each compound.a. HNO2(aq) b. B2Cl2c. BaCl2 d. CrCl3 Inorganic Nomenclature Flowchart IONIC Metal and nonmetal Metal forms one type of ion only. name of base name of cation anion (nonmetal) (metal) + -ide Example: Cal₂ calcium iodide name
Write the formula for each acid.a. Phosphoric acidb. Hydrocyanic acidc. Chlorous acid
Refer to the nomenclature flowchart (Figure 3.11) to name each compound.a. KClO3 b. I2O5c. PbSO4 Inorganic Nomenclature Flowchart IONIC Metal and nonmetal Metal forms one type of ion only. name of base name of cation anion (nonmetal) (metal) + -ide Example: Cal₂ calcium iodide name
Refer to the nomenclature flowchart (Figure 3.11) to name each compound.a. XeO3 b. KClO c. CoSO4 Inorganic Nomenclature Flowchart IONIC Metal and nonmetal Metal forms one type of ion only. name of base name of cation anion (nonmetal) (metal) + -ide Example: Cal₂ calcium iodide name
Calculate the formula mass for each compound.a. NO2b. C4H10c. C6H12O6 d. Cr(NO3)3
Calculate the formula mass for each compound.a. MgBr2 b. HNO2c. CBr4 d. Ca(NO3)2
Calculate the number of moles in each sample.a. 72.5 g CCl4b. 12.4 g C12H22O11c. 25.2 kg C2H2d. 12.3 g dinitrogen monoxide
Calculate the mass of each sample.a. 15.7 mol HNO3b. 1.04 * 10-3 mol H2O2c. 72.1 mmol SO2d. 1.23 mol xenon difluoride
Determine the number of moles (of molecules or formula units) in each sample.a. 25.5 g NO2b. 1.25 kg CO2c. 38.2 g KNO3d. 155.2 kg Na2SO4
Determine the number of moles (of molecules or formula units) in each sample.a. 55.98 g CF2Cl2b. 23.6 kg Fe(NO3)2c. 0.1187 g C8H18d. 195 kg CaO
How many molecules are in each sample?a. 6.5 g H2Ob. 389 g CBr4c. 22.1 g O2d. 19.3 g C8H10
How many molecules (or formula units) are in each sample?a. 85.26 g CCl4b. 55.93 kg NaHCO3c. 119.78 g C4H10d. 4.59 * 105 g Na3PO4
Calculate the mass (in g) of each sample.a. 5.94 * 1020 SO3 moleculesb. 2.8 * 1022 H2O moleculesc. 1 glucose molecule (C6H12O6)
Calculate the mass (in g) of each sample.a. 4.5 * 1025 O3 moleculesb. 9.85 * 1019 CCl2F2 moleculesc. 1 water molecule
A sugar crystal contains approximately 1.8 * 1017 sucrose (C12H22O11) molecules. What is its mass in mg?
A salt crystal has a mass of 0.12 mg. How many NaCl formula units does it contain?
Calculate the mass percent composition of carbon in each carbon-containing compound.a. CH4 b. C2H6 c. C2H2 d. C2H5Cl
Calculate the mass percent composition of nitrogen in each nitrogen- containing compound.a. N2O b. NO c. NO2 d. HNO3
Most fertilizers consist of nitrogen-containing compounds such as NH3, CO(NH2)2, NH4NO3, and (NH4)2SO4. Plants use the nitrogen content in these compounds for protein synthesis. Calculate the mass percent composition of nitrogen in each of the fertilizers listed. Which fertilizer has the highest
Combustion analysis of naphthalene, a hydrocarbon used in mothballs, produces 8.80 g CO2 and 1.44 g H2O. Calculate the empirical formula of naphthalene.
Iron in the earth is in the form of iron ore. Common ores include Fe2O3 (hematite), Fe3O4 (magnetite), and FeCO3 (siderite).Calculate the mass percent composition of iron for each of these iron ores. Which ore has the highest iron content?
Copper(II) fluoride contains 37.42% F by mass. Calculate the mass of fluorine (in g) in 55.5 g of copper(II) fluoride.
Write a ratio showing the relationship between the molar amounts of each element for each compound. a. b. J
The American Dental Association recommends that an adult female should consume 3.0 mg of fluoride (F–) per day to prevent tooth decay. If the fluoride is consumed in the form of sodium fluoride (45.24% F), what amount of sodium fluoride contains the recommended amount of fluoride?
Write a ratio showing the relationship between the molar amounts of each element for each compound. a. b.
Determine the number of moles of hydrogen atoms in each sample.a. 0.0885 mol C4H10 b. 1.3 mol CH4c. 2.4 mol C6H12 d. 1.87 mol C8H18
Determine the number of moles of oxygen atoms in each sample.a. 4.88 mol H2O2 b. 2.15 mol N2Oc. 0.0237 mol H2CO3 d. 24.1 mol CO2
Calculate the mass (in grams) of sodium in 8.5 g of each sodium-containing food additive.a. NaCl (table salt)b. Na3PO4 (sodium phosphate)c. NaC7H5O2 (sodium benzoate)d. Na2C6H6O7 (sodium hydrogen citrate)
The 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.
The 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.
A 0.77-mg sample of nitrogen reacts with chlorine to form 6.61 mg of the chloride. Determine the empirical formula of nitrogen chloride.
From the given empirical formula and molar mass, find the molecular formula of each compound.a. C6H7N,186.24 g/mol b. C2HCl,181.44 g/molc. C5H10NS2, 296.54 g/mol
From the given molar mass and empirical formula of several compounds, find the molecular formula of each compound.a. C4H9,114.22 g/mol b. CCl, 284.77 g/molc. C3H2N, 312.29 g/mol
Combustion analysis of a hydrocarbon produces 33.01 g CO2 and 13.51 g H2O. Calculate the empirical formula of the hydrocarbon.
The foul odor of rancid butter is due largely to butyric acid, a compound containing carbon, hydrogen, and oxygen. Combustion analysis of a 4.30-g sample of butyric acid produces 8.59 g CO2 and 3.52 g H2O. Determine the empirical formula of butyric acid.
Tartaric acid is the white, powdery substance that coats tart candies such as Sour Patch Kids. Combustion analysis of a 12.01-g sample of tartaric acid—which contains only carbon, hydrogen, and oxygen—produces 14.08 g CO2 and 4.32 g H2O. Determine the empirical formula of tartaric acid.
Classify each compound as organic or inorganic.a. CaCO3b. C4H8c. C4H6O6d. LiF
Classify each hydrocarbon as an alkane, alkene, or alkyne. a. H₂C=CH-CH3 b. H3C-CH₂-CH3 c. HC=C-CH3 d. H3C-CH₂-CH₂-CH3
Classify each hydrocarbon as an alkane, alkene, or alkyne. a. HC=CH b. H3C-CH=CH-CH3 CH3 c. H;C—CH…CH3 d. H3C-C=C-CH3
Classify each compound as organic or inorganic.a. C8H18b. CH3NH2c. CaOd. FeCO3
Write the formula based on the name, or the name based on the formula, for each hydrocarbon.a. Propaneb. CH3CH2CH3c. Octaned. CH3CH2CH2CH2CH3
Classify each organic compound as a hydrocarbon or a functionalized hydrocarbon. For functionalized hydrocarbons, identify the compound’s family. H3C-CH₂OH a. b. H3C-CH3 O || C CH₂ - CH3 c. H3C d. H₂C-NH₂
Write the formula based on the name, or the name based on the formula, for each hydrocarbon.a. CH3CH3 b. Pentanec. CH3CH2CH2CH2CH2CH3 d. Heptane
Classify each organic compound as a hydrocarbon or a functionalized hydrocarbon. For functionalized hydrocarbons, identify the compound’s family. a. H3C-CH₂-C-OH CH3 C. H₂C-C-CH3 CH3 || b. H3C-CH d. H3C-CH₂-O-CH3
How many molecules of ethanol (C2H5OH) (the alcohol in alcoholic beverages) are present in 145 mL of ethanol? The density of ethanol is 0.789 g/cm3.
A drop of water has a volume of approximately 0.05 mL. How many water molecules does it contain? The density of water is 1.0 g/cm3.
Determine the chemical formula of each compound and then use it to calculate the mass percent composition of each constituent element.a. Potassium chromateb. Lead(II) phosphatec. Sulfurous acidd. Cobalt(II) bromide
Determine the chemical formula of each compound and then use it to calculate the mass percent composition of each constituent element.a. Perchloric acidb. Phosphorus pentachloridec. Nitrogen triiodided. Carbon dioxide
A Freon leak in the air-conditioning system of an old car releases 25 g of CF2Cl2 per month. What mass of chlorine does this car emit into the atmosphere each year?
A Freon leak in the air-conditioning system of a large building releases 12 kg of CHF2Cl per month. If the leak is allowed to continue, how many kilograms of Cl will be emitted into the atmosphere each year?
A metal (M) forms a compound with the formula MCl3. If the compound contains 65.57% Cl by mass, what is the identity of the metal?
A metal (M) forms an oxide with the formula M2O. If the oxide contains 16.99% O by mass, what is the identity of the metal?
Estradiol is a female sexual hormone that is responsible for the maturation and maintenance of the female reproductive system.Elemental analysis of estradiol gives the following mass percent composition: C 79.37%, H 8.88%, O 11.75%. The molar mass of estradiol is 272.37 g/mol. Find the molecular
Fructose is a common sugar found in fruit. Elemental analysis of fructose gives the following mass percent composition:C 40.00%, H 6.72%, O 53.28%. The molar mass of fructose is 180.16 g/mol. Find the molecular formula of fructose.
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