Respuesta :
Lets assume that 100 grams of the compound are present.
Carbon mass: 88.14 g
Hydrogen mass: 11.86 g
Moles carbon: 88.14/12 = 7.34
Moles hydrogen: 11.86/1 = 11.86
The moles of carbon are 7.34 and the moles of hydrogen are 11.86.
Carbon mass: 88.14 g
Hydrogen mass: 11.86 g
Moles carbon: 88.14/12 = 7.34
Moles hydrogen: 11.86/1 = 11.86
The moles of carbon are 7.34 and the moles of hydrogen are 11.86.
[tex]$\boxed{{\text{7}}{\text{.345mol}}}$[/tex] of carbon and [tex]$\boxed{{\text{11}}{\text{.86mol}}}$[/tex] of hydrogen is present in the given compound.
Further Explanation:
Mole is a measure of the amount of substance. It is defined as the mass of a substance that has the same number of fundamental units as there are atoms in 12 g of carbon-12. Such fundamental units can be atoms, molecules or formula units.
Consider the mass of the compound to be 100 g.
The formula to calculate the mass of carbon in the compound is calculated as follows:
[tex]${\text{Mass of carbon}}=\left({\frac{{\% \;{\text{of carbon}}}}{{100\%}}}\right)\left({{\text{Mass of compound}}}\right)$[/tex] …… (1)
The % of carbon in the compound is 88.14 %.
The mass of the compound is 100 g.
Substitute these values in equation (1).
[tex]$\align{{\text{Mass of carbon}}&=\left({\frac{{88.14\,\;\%}}{{100\%}}}\right)\left({{\text{100g}}}\right)\cr&={\text{88}}{\text{.14}}\;{\text{g}}\cr}$[/tex]
The formula to calculate the mass of hydrogen in the compound is calculated as follows:
[tex]${\text{Mass of hydrogen}}=\left({\frac{{\% \;{\text{of hydrogen}}}}{{100\%}}}\right)\left({{\text{Mass of hydrogen}}}\right)$[/tex] …… (2)
The % of hydrogen in the compound is 11.86 %.
The mass of the compound is 100 g.
Substitute these values in equation (2).
[tex]$\align{{\text{Mass of hydrogen}}&=\left({\frac{{11.86\,\;\%}}{{100\%}}}\right)\left({{\text{100g}}}\right)\cr&={\text{11}}{\text{.86}}\;{\text{g}}\cr}$[/tex]
The formula to calculate the moles of carbon is as follows:
[tex]{\text{Moles of carbon}}=\frac{{{\text{Given mass of carbon}}}}{{{\text{Molar mass of carbon}}}}[/tex]
(3)
The given mass of carbon is 88.14 g.
Molar mass of carbon is 12 g/mol.
Substitute these values in equation (3).
[tex]$\align{{\text{Moles of carbon}}&=\left( {88.14\;{\text{g}}}\right)\left({\frac{{1\;{\text{mol}}}}{{12\;{\text{g}}}}}\right)\cr&={\text{7}}{\text{.345 mol}}\cr}$[/tex]
The formula to calculate the moles of hydrogen is as follows:
[tex]{\text{Moles of hydrogen}}=\frac{{{\text{Given mass of hydrogen}}}}{{{\text{Molar mass of hydrogen}}}}[/tex]
…… (4)
Given mass of hydrogen is 11.86 g.
Molar mass of hydrogen is 1 g/mol.
Substitute these values in equation (4).
[tex]$\align{{\text{Moles of hydrogen}}&=\left( {11.86\;{\text{g}}}\right)\left({\frac{{1\;{\text{mol}}}}{{1\;{\text{g}}}}}\right)\cr&={\text{11}}{\text{.86mol}}\cr}$[/tex]
Learn more:
1. Calculate the mass of ammonia: https://brainly.com/question/6078553
2. What is the molar mass of phenol? https://brainly.com/question/5671083
Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Mole concept
Keywords: mole, carbon, hydrogen, mass, mass of hydrogen, mass of compound, mass of carbon, molar mass, molar mass of carbon, molar mass of hydrogen, 12 g/mol, 1 g/mol, 11.86 mol, 7.345 mol, compound.
