Basic Chemistry
6th Edition
ISBN: 9780134878119
Author: Timberlake, Karen C. , William
Publisher: Pearson,
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 7.5, Problem 44PP
Calculate the empirical formula for each of the following:
a. 2.90 g of Ag and 0.430 g of S
b. 2.22 g of Na and 0.774 g of O
c. 2.11 g of Na, 0.0900 g of H, 2.94 g of S, and 5.86 g of O
d. 5.52 g of K, 1.45 g of P, and 3.00 g of O
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Determine the empirical and molecular formula of the following compounds:
a. limestone with a molecular mass of 100g, containing 40g of calcium, 12g of carbon, and 48g of oxygen
b. a hydrocarbon with a molecular mass of 70g, containing 85.7g of carbon and 14.3g of hydrogen
C. Sodium nitrite with a molecular mass of 69g, containing 33.32% Na, 20.30% N, and 46.38% O, which is used to preserve bacon and other meat
d. dichloroethane, a compound containing C, H, and Cl which is often used for dry cleaning with a molecular weight of 99g, containing 24.3% carbon and 71.6% chlorine
40. Calculate the number of moles in each of the followine
of NaCl
a. 32.3 grams
b. 11.6 grams of CO2
c. 508.3 grams of C,H,
42. Calculate the number of moles in each of the following:
a. 123.5 g of KCIO
b. 17.3 g of H,
c. 11.6 mg of Ca(CIO,)2
44. Convert each of the following to moles and to atoms:
a. 18.7 grams of calcium metal
b. 51.9 grams of tellurium, Te
c. 178.4 grams of uranium, U
III. Find the number of moles of the following:
A.56.1 g of Zn(C₂H302)2
B.232 g of Na3PO4
Chapter 7 Solutions
Basic Chemistry
Ch. 7.1 - What is a mole?Ch. 7.1 - What is Avogadro’s number?Ch. 7.1 - Calculate each of the following: a. number of C...Ch. 7.1 - Calculate each of the following: a. number of Li...Ch. 7.1 - Calculate each of the following quantities in 2.00...Ch. 7.1 - Calculate each of the following quantities in...Ch. 7.1 - Quinine, C20H24N2O2 , is a component of tonic...Ch. 7.1 - Aluminum sulfate, Al2(SO4)3 , is used in some...Ch. 7.1 - Naproxen is used to treat pain and inflammation...Ch. 7.1 - Benadryl is an over-the-counter drug used to treat...
Ch. 7.2 - Calculate the molar mass for each of the...Ch. 7.2 - Calculate the molar mass for each of the...Ch. 7.2 - Calculate the molar mass for each of the...Ch. 7.2 - Calculate the molar mass for each of the...Ch. 7.2 - Calculate the molar mass for each of the...Ch. 7.2 - Calculate the molar mass for each of the...Ch. 7.2 - Calculate the molar mass for each of the...Ch. 7.2 - Calculate the molar mass for each of the...Ch. 7.2 - Calculate the molar mass for each of the...Ch. 7.2 - Calculate the molar mass for each of the...Ch. 7.3 - Calculate the mass, in grams, for each of the...Ch. 7.3 - Calculate the mass, in grams, for each of the...Ch. 7.3 - Calculate the mass, in grams, in 0.150 mol of each...Ch. 7.3 - Calculate the mass, in grams, in 2.28 mol of each...Ch. 7.3 - Calculate the number of moles in each of the...Ch. 7.3 - Calculate the number of moles in each of the...Ch. 7.3 - Calculate the number of moles in 25.0 g of each of...Ch. 7.3 - Calculate the number of moles in 4.00 g of each of...Ch. 7.3 - Calculate the mass, in grams, of C in each of the...Ch. 7.3 - Calculate the mass, in grams, of N in each of the...Ch. 7.3 - Propane gas, C3H8 , is used as a fuel for many...Ch. 7.3 - Allyl sulfide, (C3H5)2S , gives garlic, onions,...Ch. 7.3 - a. The compound MgSO4 , Epsom salts, is used to...Ch. 7.3 - Prob. 34PPCh. 7.3 - Prob. 35PPCh. 7.3 - Prob. 36PPCh. 7.4 - Calculate the mass percent composition of each of...Ch. 7.4 - Calculate the mass percent composition of each of...Ch. 7.4 - Prob. 39PPCh. 7.4 - Prob. 40PPCh. 7.4 - Prob. 41PPCh. 7.4 - Calculate the mass percent of S in each of the...Ch. 7.5 - Calculate the empirical formula for each of the...Ch. 7.5 - Calculate the empirical formula for each of the...Ch. 7.5 - Calculate the empirical formula for each of the...Ch. 7.5 - Calculate the empirical formula for each of the...Ch. 7.6 - Write the empirical formula for each of the...Ch. 7.6 - Prob. 48PPCh. 7.6 - The carbohydrate fructose found in honey and...Ch. 7.6 - Caffeine has an empirical formula of C4H5N2O . If...Ch. 7.6 - Prob. 51PPCh. 7.6 - Glyoxal, used in textiles; maleic acid, used to...Ch. 7.6 - Prob. 53PPCh. 7.6 - Prob. 54PPCh. 7.6 - Vanillic acid contains 57.14% C, 4.80% H, and...Ch. 7.6 - Lactic acid, the substance that builds up in...Ch. 7.6 - A sample of nicotine, a poisonous compound found...Ch. 7.6 - Adenine, a nitrogen-containing compound found in...Ch. 7.6 - Clavulanic acid has a molecular formula of C8H9NO5...Ch. 7.6 - Phenylpropanolamine (PPA) is used to treat urinary...Ch. 7 - The chapter sections to review are shown in...Ch. 7 - The chapter sections to review are shown in...Ch. 7 - The chapter sections to review are shown in...Ch. 7 - Prob. 64UTCCh. 7 - Prob. 65APPCh. 7 - Calculate the mass, in grams, of Cu in each of the...Ch. 7 - Prob. 67APPCh. 7 - Calculate the mass percent composition for each of...Ch. 7 - Prob. 69APPCh. 7 - Prob. 70APPCh. 7 - A mixture contains 0.250 mol of Mn2O3 and 20.0 g...Ch. 7 - A mixture contains 4.001023 molecules of PCl3 and...Ch. 7 - Prob. 73APPCh. 7 - Prob. 74APPCh. 7 - Prob. 75APPCh. 7 - Prob. 76APPCh. 7 - Prob. 77APPCh. 7 - Prob. 78APPCh. 7 - Calculate the molar mass for each of the...Ch. 7 - Calculate the molar mass for each of the...Ch. 7 - Aspirin, C9H8O4 , is used to reduce inflammation...Ch. 7 - Ammonium sulfate, (NH4)2SO4 , is used in...Ch. 7 - Prob. 83APPCh. 7 - Prob. 84APPCh. 7 - Oleic acid, a component of olive oil, is 76.54% C,...Ch. 7 - Prob. 86APPCh. 7 - Prob. 87CPCh. 7 - Prob. 88CPCh. 7 - Prob. 89CPCh. 7 - The following problems are related to the topics...Ch. 7 - For parts a to f, consider the loss of electrons...Ch. 7 - A sterling silver bracelet, which is 92.5% silver...Ch. 7 - Prob. 9CICh. 7 - The active ingredient in an antacid tablet is...Ch. 7 - Oseltamivir, C16H28N2O4 , is a drug that is used...Ch. 7 - Prob. 12CI
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- A chemical compound is analyzed for its elemental composition, and is found to contain 57.14% carbon, 4.80% hydrogen, and 38.06% oxygen. The empirical formula for this chemical compound is: A. C2H2O B. CH2O C. C2H4O D. C2H4O2 E. C4H6Oarrow_forwardCalculate the empirical formula for each of the following substance Part A. 3.57 g of N and 2.04 g of O Part B. 7.00 g of C and 1.75 g of H Part C. 0.175 g of H, 2.44 g of N, and 5.59 g of O Part D. 2.06 g of Ca, 1.65 g of S, and 3.29 g of O Express your answer as a chemical formula.arrow_forward4. How many moles of Vitamin E ( the formula is written down) are present in 10.0 g of Vitamin E? Vita min E : C29H5002 3.39x10-2mol 2.07x10-2mol O 2.32x10-2molarrow_forward
- 1. The number of atoms in 2.0 mol of nitrogen gas, N2, is: a. 1.8 x 1024 b. 2.4 x 1025 c. 1.2 x 1024 d. 2.4 x 1024 e. 4.0 x 1023 2. The molar mass of a compound with the empirical formula CH₂O has a mass of approximately 90 g. What is the molecular formula of the compound? a. C4H₂O4 b. C₂H6O₂ c. C₂H₂O6 d. CzH6O3 €. CHO 3. A sample of hexane, C6H₁4, contains 3.0 x 1023 molecules of hexane. How many atoms are in the sample? a. 36 x 1024 b. 1.8 x 1023 c. 3.6 x 1024 d. 6.0 x 1024 e. 3.0 x 1023 4. Examine the following formulas. Which formula is an empirical formula? a. C₂H4 b. CsHo C. CH₂ d. C₂H₂ e. H₂O₂ 5. What is the molar mass of ammonium sulfite? a. 116.12g/mol b. 68.17g/mol c. 50.12g/mol d. 132.17g/molarrow_forwardA 1.375 g sample of mannitol, a sugar found in seaweed, is burned completely in oxygen to give 1.993 g of carbon dioxide and 0.9519 g of water. The empirical formula of mannitol is Select one: a. C,H,03 b. CHO c. CH,0 d. CH,03 e. C,H,0arrow_forwardCalculate the number of mol corresponding to:a. 0.10 g Ca b. 4.00 g Fe c. 2.00 kg N2arrow_forward
- 3. It is found a certain sample of a compound contains 23.0g of sodium and 35.5g of chlorine. a. What is the percent composition of this compound? b. How much chlorine would be needed to make 7.0g of this compound? 4. Determine the empirical formula for the following compounds a. A poisonous gas, cyanogen, is 46.14% carbon and 53.8% nitrogen. What is the empirical formula of cyanogen? b. A fuel is 85.59% carbon and 14.41% hydrogen. Determine the empirical formula.arrow_forward6.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 78. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product carbon dioxide water mass 22.00 g 4.50 g 0/5 Use this information to find the molecular formula of X. Damilola V ?arrow_forwardWhich contains the most moles of carbon? A. 23.9 grams of Co2 B. 9.4 grams of C3H4 C. 71.016 grams of C2Cl6arrow_forward
- A 0.8715 g sample of sorbic acid, a compound first obtained from the berries of a certain ash tree, is burned completely in oxygen to give 2.053 g of carbon dioxide and 0.5601 g of water. The empirical formula of sorbic acid is Select one: a. C2H4O2 b. C3H4O2 c. CH2O d. CH4O3 e. C3H4Oarrow_forwardSUBJECT: CHEMISTRYShow step by step solution:A. Using mole ratio, convert each of the following grams to moles.1. 11.0 g C6H12O6 - 2. 18.0 g Ca(OH)2 B. Using mole ratio, convert each of the following moles to grams.1. 164.21 moles N2O4 2. 6.65 moles H3PO4 AVOGADRO’S NUMBER1. How many moles of gold are there in a 8.21x1016 atoms of gold? 2. How many molecules are there in 8.00 moles of glucose, C6H12O6? 3. How many moles are there in 1.20x1024 formula units of Calcium iodide? 4. How many oxygen molecules are present in 3.9 g of Oxygen (O2) PERCENT COMPOSITIONFind the percent composition of all the elements in the following compounds;1. Mg(NO3)2 2. CuBr EMPIRICAL FORMULA1. Find the empirical formula for a compound which contains 32.8% chromium and 67.2% chlorine. MOLECULAR FORMULA1. The empirical formula of a compound phosphorous and oxygen was found to be P2O5.The molar mass of this compound is 283.88 g/mol. What is the compound’s molecular formula?arrow_forwardII. Find the Empirical and Molecular formulas given the percent composition or masses of: B. 81.8 g of C and 18.2 g of H that has a molar mass of 132.0 g/mol. C. 20.2% Na, 37.6 % S, and 42.2 %0 that has a molar mass of 682.8 g/mol.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningLiving By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Living By Chemistry: First Edition Textbook
Chemistry
ISBN:9781559539418
Author:Angelica Stacy
Publisher:MAC HIGHER
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Step by Step Stoichiometry Practice Problems | How to Pass ChemistryMole Conversions Made Easy: How to Convert Between Grams and Moles; Author: Ketzbook;https://www.youtube.com/watch?v=b2raanVWU6c;License: Standard YouTube License, CC-BY