Skip to main content

Science Chemistry Chemistry: An Introduction to General, Organic, and Biological Chemistry, Books a la Carte Edition & Modified MasteringChemistry with Pearson eText -- ValuePack Access Card Package

The available mass can be calculated from the available moles if the molar mass of the compound is known. Concept introduction: A mole is defined as an amount of substance that has the same number of atoms as there are in 12 grams of Carbon. There are 6.022 x 10 23 atoms in 12 grams of Carbon The molar mass of a compound is the sum of the masses of the elements that form it. The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. To determine: The mass of different compounds Solution: a) 190 .6 grams b) 273 grams c) 230 grams d) 43 .92 grams Step 1: To determine: The mass of 2 moles of M g C l 2 . To find the molar mass of the compound it is required to multiply the atomic weight of each element by the number of atoms of that element in the molecule and add all the masses. The atomic weight of any element can be found in the periodic table. 1 mole of M g C l 2 has 1 mole of Mg and 2 moles of Cl. Mass of 1 mole of Mg 1 mole of Mg x 24 .3 grams of Mg 1 mole of Mg = 24.3 grams of Mg Mass of 2 moles of Cl 2 moles of Cl x 35 .5 grams of Cl 1 mole of Cl = 71 grams of Cl Add all the masses of the different elements to find the molar mass of M g C l 2 : mass of Mg + mass of Cl = 24 .3 + 71 = 95 .3 grams mole The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. Using this definition, it is possible to calculate the mass of Magnesium Chloride: mass = moles x molar mass mass of Magnesium Chloride = 2 moles x 95 .3 grams mole = 190.6 grams Step 2: To determine: The mass of 3.5 moles of C 6 H 6 . To find the molar mass of the compound it is required to multiply the atomic weight of each element by the number of atoms of that element in the molecule and add all the masses. The atomic weight of any element can be found in the periodic table. 1 mole of C 6 H 6 has 6 moles of C and 6 moles of H. Mass of 6 moles of C 6 moles of C x 12 grams of C 1 mole of C = 72 grams of C Mass of 6 moles of H 6 moles of H x 1 grams of H 1 mole of H = 6 grams of H Add all the masses of the different elements to find the molar mass of C 6 H 6 : mass of C + mass of H = 72 + 6 = 78 grams mole The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. Using this definition, it is possible to calculate the mass of C 6 H 6 : mass = moles x molar mass mass of C 6 H 6 = 3 .5 moles x 78 grams mole = 273 grams Step 3: To determine: The mass of 5 moles of C 2 H 6 O . To find the molar mass of the compound it is required to multiply the atomic weight of each element by the number of atoms of that element in the molecule and add all the masses. The atomic weight of any element can be found in the periodic table. 1 mole of C 2 H 6 O has 2 moles of C, 6 moles of H and 1 mole of O. Mass of 2 moles of C 2 moles of C x 12 grams of C 1 mole of C = 24 grams of C Mass of 6 moles of H: 6 moles of H x 1 gram of H 1 mole of H = 6 grams of H Mass of 1 mole of O 1 mole of O x 16 grams of O 1 mole of O = 16 grams of O Add all the masses of the different elements to find the molar mass of C 2 H 6 O : mass of C + mass of H + mass of O = 24 + 6 + 16 = 46 grams mole The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. Using this definition, it is possible to calculate the mass of C 2 H 6 O : mass = moles x molar mass mass of C 2 H 6 O = 5 moles x 46 grams mole = 230 grams Step 4: To determine: The mass of 0.488 moles of C 3 H 6 O 3 . To find the molar mass of the compound it is required to multiply the atomic weight of each element by the number of atoms of that element in the molecule and add all the masses. The atomic weight of any element can be found in the periodic table. 1 mole of C 3 H 6 O 3 has 3 moles of C, 6 moles of H and 3 moles of O. Mass of 3 moles of C 3 moles of C x 12 grams of C 1 mole of C = 36 grams of C Mass of 6 moles of H: 6 moles of H x 1 gram of H 1 mole of H = 6 grams of H Mass of 3 moles of O 3 moles of O x 16 grams of O 1 mole of O = 48 grams of O Add all the masses of the different elements to find the molar mass of C 3 H 6 O 3 : mass of C + mass of H + mass of O = 36 + 6 + 48 = 90 grams mole The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. Using this definition, it is possible to calculate the mass of C 3 H 6 O 3 : mass = moles x molar mass mass of C 3 H 6 O 3 = 0 .488 moles x 90 grams mole = 43.92 grams Conclusion: The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. If the moles and the molar mass of a compound are known, then it is possible to calculate the mass of that element.

The available mass can be calculated from the available moles if the molar mass of the compound is known. Concept introduction: A mole is defined as an amount of substance that has the same number of atoms as there are in 12 grams of Carbon. There are 6.022 x 10 23 atoms in 12 grams of Carbon The molar mass of a compound is the sum of the masses of the elements that form it. The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. To determine: The mass of different compounds Solution: a) 190 .6 grams b) 273 grams c) 230 grams d) 43 .92 grams Step 1: To determine: The mass of 2 moles of M g C l 2 . To find the molar mass of the compound it is required to multiply the atomic weight of each element by the number of atoms of that element in the molecule and add all the masses. The atomic weight of any element can be found in the periodic table. 1 mole of M g C l 2 has 1 mole of Mg and 2 moles of Cl. Mass of 1 mole of Mg 1 mole of Mg x 24 .3 grams of Mg 1 mole of Mg = 24.3 grams of Mg Mass of 2 moles of Cl 2 moles of Cl x 35 .5 grams of Cl 1 mole of Cl = 71 grams of Cl Add all the masses of the different elements to find the molar mass of M g C l 2 : mass of Mg + mass of Cl = 24 .3 + 71 = 95 .3 grams mole The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. Using this definition, it is possible to calculate the mass of Magnesium Chloride: mass = moles x molar mass mass of Magnesium Chloride = 2 moles x 95 .3 grams mole = 190.6 grams Step 2: To determine: The mass of 3.5 moles of C 6 H 6 . To find the molar mass of the compound it is required to multiply the atomic weight of each element by the number of atoms of that element in the molecule and add all the masses. The atomic weight of any element can be found in the periodic table. 1 mole of C 6 H 6 has 6 moles of C and 6 moles of H. Mass of 6 moles of C 6 moles of C x 12 grams of C 1 mole of C = 72 grams of C Mass of 6 moles of H 6 moles of H x 1 grams of H 1 mole of H = 6 grams of H Add all the masses of the different elements to find the molar mass of C 6 H 6 : mass of C + mass of H = 72 + 6 = 78 grams mole The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. Using this definition, it is possible to calculate the mass of C 6 H 6 : mass = moles x molar mass mass of C 6 H 6 = 3 .5 moles x 78 grams mole = 273 grams Step 3: To determine: The mass of 5 moles of C 2 H 6 O . To find the molar mass of the compound it is required to multiply the atomic weight of each element by the number of atoms of that element in the molecule and add all the masses. The atomic weight of any element can be found in the periodic table. 1 mole of C 2 H 6 O has 2 moles of C, 6 moles of H and 1 mole of O. Mass of 2 moles of C 2 moles of C x 12 grams of C 1 mole of C = 24 grams of C Mass of 6 moles of H: 6 moles of H x 1 gram of H 1 mole of H = 6 grams of H Mass of 1 mole of O 1 mole of O x 16 grams of O 1 mole of O = 16 grams of O Add all the masses of the different elements to find the molar mass of C 2 H 6 O : mass of C + mass of H + mass of O = 24 + 6 + 16 = 46 grams mole The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. Using this definition, it is possible to calculate the mass of C 2 H 6 O : mass = moles x molar mass mass of C 2 H 6 O = 5 moles x 46 grams mole = 230 grams Step 4: To determine: The mass of 0.488 moles of C 3 H 6 O 3 . To find the molar mass of the compound it is required to multiply the atomic weight of each element by the number of atoms of that element in the molecule and add all the masses. The atomic weight of any element can be found in the periodic table. 1 mole of C 3 H 6 O 3 has 3 moles of C, 6 moles of H and 3 moles of O. Mass of 3 moles of C 3 moles of C x 12 grams of C 1 mole of C = 36 grams of C Mass of 6 moles of H: 6 moles of H x 1 gram of H 1 mole of H = 6 grams of H Mass of 3 moles of O 3 moles of O x 16 grams of O 1 mole of O = 48 grams of O Add all the masses of the different elements to find the molar mass of C 3 H 6 O 3 : mass of C + mass of H + mass of O = 36 + 6 + 48 = 90 grams mole The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. Using this definition, it is possible to calculate the mass of C 3 H 6 O 3 : mass = moles x molar mass mass of C 3 H 6 O 3 = 0 .488 moles x 90 grams mole = 43.92 grams Conclusion: The number of available moles is the ratio of the mass of a compound to the molar mass of the compound. If the moles and the molar mass of a compound are known, then it is possible to calculate the mass of that element.

Chemistry: An Introduction to General, Organic, and Biological Chemistry, Books a la Carte Edition & Modified MasteringChemistry with Pearson eText -- ValuePack Access Card Package

Chemistry: An Introduction to General, Organic, and Biological Chemistry, Books a la Carte Edition & Modified MasteringChemistry with Pearson eText -- ValuePack Access Card Package

1st Edition

ISBN: 9780133899573

Author: Karen C. Timberlake

Publisher: PEARSON

See similar textbooks

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

Blurred answer

Chapter 7.2, Problem 7.15QAP

Chapter 7.2, Problem 7.17QAP

Students have asked these similar questions

Laminar compounds are characterized by havinga) a high value of the internal surface of the solid.b) a high adsorption potential.

Intercalation compounds have their sheetsa) negatively charged.b) positively charged.

Indicate whether the following two statements are correct or not:- Polythiazine, formed by N and S, does not conduct electricity- Carbon can have a specific surface area of 3000 m2/g

Chapter 7 Solutions

Chemistry: An Introduction to General, Organic, and Biological Chemistry, Books a la Carte Edition & Modified MasteringChemistry with Pearson eText -- ValuePack Access Card Package

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 200...Ch. 7.1 - Calculate each of the following quantities in...Ch. 7.1 - Prob. 7.7QAP Ch. 7.1 - Aluminum sulphate, Al2SO43 , is used in some...Ch. 7.2 - Prob. 7.9QAP Ch. 7.2 - Prob. 7.10QAP

Ch. 7.2 - Prob. 7.11QAP Ch. 7.2 - Prob. 7.12QAP Ch. 7.2 - Prob. 7.13QAP Ch. 7.2 - Prob. 7.14QAP Ch. 7.2 - Prob. 7.15QAP Ch. 7.2 - Prob. 7.16QAP Ch. 7.2 - Prob. 7.17QAP Ch. 7.2 - Prob. 7.18QAP Ch. 7.2 - Prob. 7.19QAP Ch. 7.2 - Prob. 7.20QAP Ch. 7.2 - Prob. 7.21QAP Ch. 7.2 - Prob. 7.22QAP Ch. 7.2 - Prob. 7.23QAP Ch. 7.2 - Prob. 7.24QAP Ch. 7.2 - Prob. 7.25QAP Ch. 7.2 - Prob. 7.26QAP Ch. 7.3 - Determine whether each of the following chemical...Ch. 7.3 - Determine whether each of the following chemical...Ch. 7.3 - Balance each of the following chemical equations:...Ch. 7.3 - Balance each of the following chemical equations:...Ch. 7.3 - Balance each of the following chemical equations:...Ch. 7.3 - Balance each of the following chemical equations:...Ch. 7.4 - Prob. 7.33QAP Ch. 7.4 - Prob. 7.34QAP Ch. 7.4 - Prob. 7.35QAP Ch. 7.4 - Prob. 7.36QAP Ch. 7.4 - Prob. 7.37QAP Ch. 7.4 - Prob. 7.38QAP Ch. 7.5 - Prob. 7.39QAP Ch. 7.5 - Prob. 7.40QAP Ch. 7.5 - In each of the following, identify the reactant...Ch. 7.5 - In each of the following, identify the reactant...Ch. 7.5 - Prob. 7.43QAP Ch. 7.5 - Prob. 7.44QAP Ch. 7.5 - Prob. 7.45QAP Ch. 7.5 - Prob. 7.46QAP Ch. 7.6 - Write all of the mole—mole factors for each of the...Ch. 7.6 - Write all of the mole—mole factors for each of the...Ch. 7.6 - The chemical reaction of hydrogen with oxygen...Ch. 7.6 - Prob. 7.50QAP Ch. 7.6 - Carbon disulfide and carbon monoxide are produced...Ch. 7.6 - Prob. 7.52QAP Ch. 7.7 - Sodium reacts with oxygen to produce sodium oxide....Ch. 7.7 - Nitrogen gas reacts with hydrogen gas to produce...Ch. 7.7 - Ammonia and oxygen react to form nitrogen and...Ch. 7.7 - Iron(III) oxide reacts with carbon to give iron...Ch. 7.7 - Nitrogen dioxide and water react to produce nitric...Ch. 7.7 - Calcium cyanamide, CaCN2 , reads with water to...Ch. 7.7 - Prob. 7.59QAP Ch. 7.7 - When the gases dihydrogen sulfide and oxygen...Ch. 7.8 - Prob. 7.61QAP Ch. 7.8 - Prob. 7.62QAP Ch. 7.8 - Classify each of the following as exothermic or...Ch. 7.8 - Classify each of the following as exothermic or...Ch. 7.8 - Classify each of the following as exothermic or...Ch. 7.8 - Classify each of the following as exothermic or...Ch. 7.8 - a. What is meant by the rate of a reaction? b. Why...Ch. 7.8 - a. How does a catalyst affect the activation...Ch. 7.8 - Prob. 7.69QAP Ch. 7.8 - How would each of the following change the rate of...Ch. 7 - Prob. 7.71UTC Ch. 7 - Using the models of the molecules (black = C,...Ch. 7 - A dandruff shampoo contains dipyrithione,...Ch. 7 - Ibuprofen, an anti-inflammatory drug in Advil, has...Ch. 7 - Prob. 7.75UTC Ch. 7 - Balance each of the following by adding...Ch. 7 - Prob. 7.77UTC Ch. 7 - Prob. 7.78UTC Ch. 7 - If blue spheres represent nitrogen atoms, purple...Ch. 7 - Prob. 7.80UTC Ch. 7 - Prob. 7.81UTC Ch. 7 - Prob. 7.82UTC Ch. 7 - Calculate the molar mass for each of the...Ch. 7 - Calculate the molar mass for each of the...Ch. 7 - How many grams are in 0.150 mole of each of the...Ch. 7 - How many grams are in 2.25 moles of each of the...Ch. 7 - How many moles are in 25.0 g of each of the...Ch. 7 - How many moles are in 4.00 g of each of the...Ch. 7 - Identify the type of reaction for each of the...Ch. 7 - Identify the type of reaction for each of the...Ch. 7 - Prob. 7.91AQAP Ch. 7 - Prob. 7.92AQAP Ch. 7 - Prob. 7.93AQAP Ch. 7 - Prob. 7.94AQAP Ch. 7 - Identify each of the following as an oxidation or...Ch. 7 - Prob. 7.96AQAP Ch. 7 - When ammonia NH3 gas reacts with fluorine gas, the...Ch. 7 - When nitrogen dioxide NO2 gas from car exhaust...Ch. 7 - Pentane gas, C5H12 undergoes combustion with...Ch. 7 - Prob. 7.100AQAP Ch. 7 - Prob. 7.101AQAP Ch. 7 - The equation for the formation of nitrogen oxide...Ch. 7 - Prob. 7.103CQ Ch. 7 - Prob. 7.104CQ Ch. 7 - Prob. 7.105CQ Ch. 7 - A toothpaste contains 0.240% by mass sodium...Ch. 7 - Prob. 7.107CQ Ch. 7 - Prob. 7.108CQ Ch. 7 - Prob. 7.109CQ Ch. 7 - Prob. 7.110CQ

Knowledge Booster

Background pattern image

Similar questions

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY

Text book image

Chemistry

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Cengage Learning

Text book image

Chemistry

ISBN:9781259911156

Author:Raymond Chang Dr., Jason Overby Professor

Publisher:McGraw-Hill Education

Text book image

Principles of Instrumental Analysis

Chemistry

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Cengage Learning

Text book image

Organic Chemistry

Chemistry

ISBN:9780078021558

Author:Janice Gorzynski Smith Dr.

Publisher:McGraw-Hill Education

Text book image

Chemistry: Principles and Reactions

Chemistry

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:Cengage Learning

Text book image

Elementary Principles of Chemical Processes, Bind...

Chemistry

ISBN:9781118431221

Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:WILEY

SEE MORE TEXTBOOKS