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Calculate the molar mass of a compound if 0.372 mol of it has a mass of 152 g.

Calculate the molar mass of a compound if 0.372 mol of it has a mass of 152 g.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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3.6 Experimental Determination of Empirical Formulas 13)The reaction of copper and sulfur at high heat creates a "copper sulfide". But does it create copper (1) sulfide or cupric sulfide? An experiment is run in which Cu is heated over high heat in a crucible, three times, in the presence of excess sulfur. The results are as follows. Mass of crucible, cover, and copper sulfide = 26.512 g Determine the formula for the "copper sulfide" created and give its name. 3.7 Chemical Reactions and Chemical Equations 14) Balance the following chemical equations by placing the correct coefficient in front of each reactant/product. Research the physical state of each and add in the phase labels. _Al4C3() + H2O() → Al(OH)3()+ ___ CH4() a) Mass Empty Crucible and cover: 24.305 g Mass Crucible and Cover and copper = 25.808 g b) c) d) C7H14() +. 02()→ CO2() + - H₂00 CaSO4() + Ca3(PO4)2()+ H2SO4()→ PC13() + H2O() → H3PO3() +. 4.5 mol H2 X _H3PO40) 15) H2 and N2 react to form NH3 by the equation: N2(g) + 3H2(g) → 2NH3 (g). If a reaction vessel initially contained 300 H₂ molecules and 150 N2 molecules, which molecules will be present in the vessel if the reaction proceeds to completion? HClO Speed Stoichiometry! Let's Focus on water _H2 + _O2 → _H₂O (Balance this first!) Moles moles Example: For the following reaction, how many moles of water can be made from 4.5 moles of hydrogen? 2 mol H₂O 2 mol H₂ How many moles of oxygen are needed to react with 3.5 moles of hydrogen? How many moles of hydrogen are needed to react with 6 moles of oxygen? How many moles of water are produced from with 12.5 moles of oxygen? How many moles of water can be made from 4.5 moles of oxygen? - 4.5 mol H2O
Transcribed Image Text:3.6 Experimental Determination of Empirical Formulas 13)The reaction of copper and sulfur at high heat creates a "copper sulfide". But does it create copper (1) sulfide or cupric sulfide? An experiment is run in which Cu is heated over high heat in a crucible, three times, in the presence of excess sulfur. The results are as follows. Mass of crucible, cover, and copper sulfide = 26.512 g Determine the formula for the "copper sulfide" created and give its name. 3.7 Chemical Reactions and Chemical Equations 14) Balance the following chemical equations by placing the correct coefficient in front of each reactant/product. Research the physical state of each and add in the phase labels. _Al4C3() + H2O() → Al(OH)3()+ ___ CH4() a) Mass Empty Crucible and cover: 24.305 g Mass Crucible and Cover and copper = 25.808 g b) c) d) C7H14() +. 02()→ CO2() + - H₂00 CaSO4() + Ca3(PO4)2()+ H2SO4()→ PC13() + H2O() → H3PO3() +. 4.5 mol H2 X _H3PO40) 15) H2 and N2 react to form NH3 by the equation: N2(g) + 3H2(g) → 2NH3 (g). If a reaction vessel initially contained 300 H₂ molecules and 150 N2 molecules, which molecules will be present in the vessel if the reaction proceeds to completion? HClO Speed Stoichiometry! Let's Focus on water _H2 + _O2 → _H₂O (Balance this first!) Moles moles Example: For the following reaction, how many moles of water can be made from 4.5 moles of hydrogen? 2 mol H₂O 2 mol H₂ How many moles of oxygen are needed to react with 3.5 moles of hydrogen? How many moles of hydrogen are needed to react with 6 moles of oxygen? How many moles of water are produced from with 12.5 moles of oxygen? How many moles of water can be made from 4.5 moles of oxygen? - 4.5 mol H2O
6) Calculate the molar mass of a compound if 0.372 mol of it has a mass of 152 g. See Problem 3.25 7) Calculate the number of ethane (C2H6) molecules in 0.334 g of ethane. See Problem 3.26 8) What is the mass in grams of a single atom of arsenic(As). See Problem 3.18 9) Calculate the mass of one arsenic atom using the mass of the proton and neutron. 3.4 Mass Spectrometry 10) Carbon has two stable isotopes, 12C and C, and fluorine has only one stable isotope, F. 13 6 19 9 6 How many peaks would you observe in the mass spectrum of the positive ion of CF4+. Assume that the ion does not break up into smaller fragments. . See Problem 3.33 (Hint: Think of how many different combinations of isotopes you could make) 3.5 Percent Composition of Compounds 11) For many years chloroform (CHC13) was used as an inhalation anesthetic in spite of the fact that it is also a toxic substance that can cause severe liver, kidney, and heart damage. Calculate the percent composition by mass of each element in this compound to four significant figures. See Problem 3.40 12) Allicin is the compound responsible for the characteristic odor of garlic. An analysis of the compound gives the following percent composition by mass: C: 44.4%, H: 6.21%, S: 39.5%, 0: 9.86% Calculate its empirical formula and molecular formula given its molar mass is 162 g/mol. See Problem 3.43
Transcribed Image Text:6) Calculate the molar mass of a compound if 0.372 mol of it has a mass of 152 g. See Problem 3.25 7) Calculate the number of ethane (C2H6) molecules in 0.334 g of ethane. See Problem 3.26 8) What is the mass in grams of a single atom of arsenic(As). See Problem 3.18 9) Calculate the mass of one arsenic atom using the mass of the proton and neutron. 3.4 Mass Spectrometry 10) Carbon has two stable isotopes, 12C and C, and fluorine has only one stable isotope, F. 13 6 19 9 6 How many peaks would you observe in the mass spectrum of the positive ion of CF4+. Assume that the ion does not break up into smaller fragments. . See Problem 3.33 (Hint: Think of how many different combinations of isotopes you could make) 3.5 Percent Composition of Compounds 11) For many years chloroform (CHC13) was used as an inhalation anesthetic in spite of the fact that it is also a toxic substance that can cause severe liver, kidney, and heart damage. Calculate the percent composition by mass of each element in this compound to four significant figures. See Problem 3.40 12) Allicin is the compound responsible for the characteristic odor of garlic. An analysis of the compound gives the following percent composition by mass: C: 44.4%, H: 6.21%, S: 39.5%, 0: 9.86% Calculate its empirical formula and molecular formula given its molar mass is 162 g/mol. See Problem 3.43
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6) Given,

Number of moles=0.372

Mass=152 g

 

To calculate,

Molar mass

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