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Calculating the Mass Percent Composition of Chloroform (CHCl?)
Chapter 3, Problem 3.38(choose chapter or problem)
For many years chloroform \((\rm{CHCl}_3)\) 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.
Questions & Answers
QUESTION:
For many years chloroform \((\rm{CHCl}_3)\) 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.
ANSWER:Step 1 of 5
Molar mass of carbon is 12.011 g/mol.
Molar mass of hydrogen is 1.00784 g/mol.
Molar mass of chlorine is 35.453 g/mol.
Molar mass of chloroform is:
\(12.011\;{\rm{g/mol}} + 1.00784\;{\rm{g/mol}} + \left( {3 \times 35.453\;{\rm{g/mol}}} \right) = 119.37784\;{\rm{g/mol}} \)
Formula of finding the composition of elements is given as:
\({\rm{Percent}}\;{\rm{composition}}\;{\rm{of}}\;{\rm{an}}\;{\rm{element}} = \dfrac{{{\rm{n}} \times {\rm{molar}}\;{\rm{mass}}\;{\rm{of}}\;{\rm{the}}\;{\rm{element}}}}{{{\rm{molar}}\;{\rm{mass}}\;{\rm{of}}\;{\rm{the}}\;{\rm{compound}}}} \times 100 \)
n is the number of moles of the element.
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Calculating the Mass Percent Composition of Chloroform (CHCl?)
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In this video, we delve into the concept of percent composition by mass, exemplified through the compound chloroform (CHCl?), which was once employed as an inhalation anesthetic despite its associated toxicity. By calculating the percent composition for each element within the compound, we gain valuable insights into its composition and its potential effects on health and properties.