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Chapter 3: Problem 40

For many years chloroform \(\left(\mathrm{CHCl}_{3}\right)\) was used as an inhalation anesthetic in spite of the fact that it is also a toxic substance that may cause severe liver, kidney, and heart damage. Calculate the percent composition by mass of this compound.

Short Answer

Expert verified
The percent composition by mass of chloroform \(\mathrm{CHCl}_{3}\) is 10.06% for Carbon, 0.84% for Hydrogen and 89.10% for Chlorine.

Step by step solution

01

Determine the molar mass

Firstly, determine the molar masses of the elements that make up chloroform: Carbon (C), Hydrogen (H) and Chlorine (Cl). These can be found on the periodic table, with Carbon's molar mass as 12.01 g/mol, Hydrogen's as 1.008 g/mol and Chlorine's as 35.45 g/mol.
02

Calculate the total molar mass

Subsequently, calculate the total molar mass of chloroform \(\mathrm{CHCl}_{3}\). This is done by adding the molar mass of Carbon, the molar mass of Hydrogen and the molar mass of Chlorine (multiplied by 3 because there are three Chlorine atoms in the compound). Thus, the total molar mass is \(12.01 g/mol + 1.008 g/mol + (3 \times 35.45 g/mol) = 119.37 g/mol.\)
03

Calculate the percent composition by mass

Lastly, calculate the percent composition by mass for each element. This is done by dividing the total molar mass of each element by the total molar mass of chloroform and then multiplying by 100%. The percent compositions are \[(12.01 g/mol/119.37 g/mol) \times 100\% = 10.06\%\] for Carbon, \[(1.008 g/mol/119.37 g/mol) \times 100\% = 0.84\%\] for Hydrogen and \[(3 \times 35.45 g/mol/119.37 g/mol) \times 100\% = 89.10\%\] for Chlorine.

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Most popular questions from this chapter

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