molar mass of MgCl2
= 24.32 + 2 x (35.45) = 95.22 g
16.4g MgCl2 x (1 mol MgCl2/95.22
g MgCl2) = 0.172 mol MgCl2
0.172 mol MgCl2 x (6.022 x 10^23/1 mol
MgCl2) = 10.36 x 10^22 atoms
Answer: The number of formula units in the given amount of magnesium chloride is [tex]1.0357\times 10^{23}[/tex]
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Given mass of magnesium chloride = 16.4 g
Molar mass of magnesium chloride = 95.2 g/mol
Putting values in above equation, we get:
[tex]\text{Moles of }MgCl_2=\frac{16.4g}{95.2g/mol}=0.172mol[/tex]
Formula units is defined as lowest whole number ratio of ions in an ionic compound. It is calculated by multiplying the number of moles by Avogadro's number which is [tex]6.022\times 10^{23}[/tex]
We are given:
Number of moles of magnesium chloride = 0.172 moles
Number of formula units = [tex]0.172\times 6.022\times 10^{23}=1.0357\times 10^{23}[/tex]
Hence, the number of formula units in the given amount of magnesium chloride is [tex]1.0357\times 10^{23}[/tex]
