Respuesta :
Answer:- [tex]1.91*10^2^3Cl[/tex] atoms.
Solution:- We have been given the grams of carbon tetrachloride and asked to calculate the number of atoms of chlorine. It is a three step conversion problem. In the first we convert the grams of carbon tetrachloride to moles of it. In second step we convert moles of carbon tetrachloride to moles of chlorine and in the third step we convert the moles of chlorine to atoms of chlorine.
For grams to mole conversion we need the molar mass of the compound. Molar mass of carbon tetrachloride is 153.82 grams per mol. If we look at the formula of carbon tetrachloride then four chlorine are present in it. It means 1 mol of carbon tetrachloride has four moles of chlorine. The calculations are as follows:
[tex]12.2gCCl_4(\frac{1molCCl_4}{153.82gCCl_4})(\frac{4molCl}{1molCCl_4})(\frac{6.02*10^2^3Clatoms}{1molCl})[/tex]
= [tex]1.91*10^2^3Cl[/tex] atoms
So, there are [tex]1.91*10^2^3Cl[/tex] atoms in 12.2 grams of [tex]CCl_4[/tex] .
There are [tex]\boxed{1.91 \times {{10}^{23}}{\text{ atoms}}}[/tex] of chlorine in 12.2 g of [tex]\text{CCl}_4[/tex].
Further Explanation:
The number of moles of [tex]\text{CCl}_4[/tex] is calculated by the following formula:
[tex]{\text{Moles of CC}}{{\text{l}}_{\text{4}}} = \dfrac{{{\text{Mass of CC}}{{\text{l}}_{\text{4}}}}}{{{\text{Molar mass of CC}}{{\text{l}}_{\text{4}}}}}[/tex] ...... (1)
The mass of [tex]\text{CCl}_4[/tex] is 12.2 g.
The molar mass of [tex]\text{CCl}_4[/tex] is 153.82 g/mol.
Substitute these values in equation (1).
[tex]\begin{aligned}{\text{Moles of CC}}{{\text{l}}_{\text{4}}} &= \frac{{{\text{12}}{\text{.2 g}}}}{{{\text{153}}{\text{.82 g/mol}}}}\\&= 0.0793{\text{ mol}}\\\end{aligned}[/tex]
The number of units that are present in one mole of the substance is determined by Avogadro’s number. It has a numerical value of [tex]{\text{6}}{\text{.022}} \times {\text{1}}{{\text{0}}^{{\text{23}}}}\;{\text{units}}[/tex]. These units can be electrons, atoms, molecules or ions, depending on the nature of the substance.
The formula of carbon tetrachloride [tex]\left( {{\text{CC}}{{\text{l}}_{\text{4}}}} \right)[/tex] indicates that one mole of [tex]\text{CCl}_4[/tex] has four moles of Cl in it.
Therefore the number of moles of chlorine can be calculated as follows:
[tex]\begin{aligned}{\text{Moles of Cl}} &= \left( {0.0793{\text{ mol CC}}{{\text{l}}_4}} \right)\left( {\frac{{4{\text{ mol Cl}}}}{{1{\text{ mol CC}}{{\text{l}}_4}}}} \right)\\&= 0.31725{\text{ mol}}\\\end{aligned}[/tex]
One mole of Cl has [tex]6.022\times10^{23}[/tex] of Cl. Therefore the number of atoms of Cl can be calculated as follows:
[tex]\begin{aligned}{\text{Atoms of Cl}} &= \left( {\frac{{6.022 \times {{10}^{23}}{\text{ atoms}}}}{{1{\text{ mol}}}}} \right)\left( {0.31725{\text{ mol}}} \right)\\&= 1.9105 \times {10^{23}}{\text{ atoms}}\\&\approx 1.91 \times {10^{23}}{\text{ atoms}}\\\end{aligned}[/tex]
Therefore there are [tex]1.91 \times {10^{23}}{\text{ atoms}}[/tex] of chlorine in 12.2 g of [tex]\text{CCCI}_4[/tex].
Learn more:
- Calculate the moles of chlorine in 8 moles of carbon tetrachloride: https://brainly.com/question/3064603
- Calculate the moles of ions in the solution: https://brainly.com/question/5950133
Answer details:
Grade: Senior School
Chapter: Mole concept
Subject: Chemistry
Keywords: chlorine, CCl4, Avogadro’s number, units, atoms, molecules, ions, electrons, 12.2 g, 153.82 g/mol, mole, 6.022*10^23 atoms, 1.91*10^23 atoms, mass, molar mass, substance, number of units, nature, 0.0793 mol, 0.31725 mol.
