The total number of moles of Cl atom present in \(2.41\times{10^{24}}\) unit of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) is \(\boxed{{\text{8}}{\text{.0 moles}}}\) .
Further explanation:
Mole is a measure of the amount of substance. Mole is the relation between the mass of the substance and molar mass of substance. It is defined as the mass of a substance in grams divided by its molar mass (g/mol).
The formula to calculate the number of moles is as follows:
\({\text{Number of moles}}\;=\;\frac{{{\text{Given mass}}\left({\text{g}}\right)}}{{{\text{molar mass}}\left( {{\text{g/mol}}}\right)}}\) ...... (1)
Also, according to Avogadro's number, the number of atoms or molecules present in the 1 mole of a substance is \(6.022\times{10^{23}}\) .
This means 1 mole of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) contains \(6.022\times{10^{23}}\) formula unit of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) .
\(1{\text{ mol}}={\text{6}}{\text{.022}}\times{\text{1}}{{\text{0}}^{23}}{\text{MgC}}{{\text{l}}_2}{\text{ formula unit}}\)
Thus, the number of moles of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) in 1 formula unit of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) is,
\(1{\text{ formula unit}}\left({{\text{MgC}}{{\text{l}}_2}}\right)=\frac{1}{{{\text{6}}{\text{.022}}\times{\text{1}}{{\text{0}}^{23}}{\text{ }}}}{\text{mol }}\left({{\text{MgC}}{{\text{l}}_2}}\right)\)
The given formula unit of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) is \(2.41\times{10^{24}}\) .
Therefore, number of moles in \(2.41\times{10^{24}}\) formula units of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) can be calculated by multiplying number of moles per unit of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) with total number of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) formula units. The calculation for moles of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) is as follows:
\(\begin{aligned}{\text{Moles of MgC}}{{\text{l}}_2}&=\left({{\text{number of moles per unit of MgC}}{{\text{l}}_{\text{2}}}} \right)\left({{\text{total number of MgC}}{{\text{l}}_{\text{2}}}{\text{\;}}}\right)\\&=\left( {\frac{1}{{{\text{6}}{\text{.022}}\times{\text{1}}{{\text{0}}^{23}}{\text{ }}}}{\text{mol}}}\right)\left({2.41\times{{10}^{24}}}\right)\\&=0.40\times10{\text{mol}}\\&=4.0\,{\text{mol}}\\\end{aligned}\)
Therefore, the number of moles of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) present in \(2.41\times{10^{24}}\) formul units is 4.0 moles.
Since each unit of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) contains 2 unit of Cl atom thus 4.0 moles of \({\text{MgC}}{{\text{l}}_{\text{2}}}\) must contains 8.0 moles of Cl atom.
Learn more:
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Answer details:
Grade: Senior school
Subject: Chemistry
Chapter: Mole concept
Keywords: Total number of Cl atom, mgcl2, 2.41x10^24, moles, Avogadro number, number of moles, molar mass, given mass, total number of atoms.
