Question

What is the total number of AlF3 molecules in a sample of AlF3 containing 3.01⋅1023 fluoride ions ?

Answer 1

1 mole of AlF3 contains 3 moles of. F-

3.011 X 10^23 F- = 0.5 mole Of Flouride

3 moles of F- present in 1 mole of AlF3

0.5moles of. F- how much mole of AlF3?

= 0.5/3 =0.1666 moles of. AlF3

molecules = 0.166xNA

Answer 2

The number of aluminium fluoride molecules having given number of fluoride ions are $1.003\times 10^{23}$

Explanation:

According to mole concept:

1 mole of a compound contains $6.022\times 10^{23}$ number of particles

1 mole of $AlF_3$ contains 1 mole of aluminium ions and 3 moles of fluoride ions

Number of fluoride ions in 1 mole of $AlF_3$ of in $6.022\times 10^{23}$ number of molecules = $(3\times 6.022\times 10^{23})=18.066\times 10^{23}$

We are given:

Number of fluoride ions = $3.01\times 10^{23}$

Applying unitary method:

$18.066\times 10^{23}$ number of fluoride ions are present in $6.022\times 10^{23}$ number of aluminium fluoride molecules

So, $3.01\times 10^{23}$ number of fluoride ions will be present in = $\frac{6.022\times 10^{23}}{18.066\times 10^{23}}\times 3.01\times 10^{23}=1.003\times 10^{23}$ number of aluminium fluoride molecules

Learn more about mole concept:

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