91Ó°ÊÓ

We are given that Ibuprofen, an anti-inflammatory drug in Advil, has the formula $C_{13}{H}_{18}{0}_2$. and we need to fine the molar mass .

We are given that the chemical formula of ibuprofen $C_{13}{H}_{18}{0}_2$and we have to find the molar mass Where $C=12,O=16,H=1$

localid="1653501132520" $\mathrm{m}=12\left(\mathrm{amu}\right)×13+16\left(\mathrm{amu}\right)×2+18×1\left(\mathrm{amu}\right)$

m = localid="1653501120432" $206\mathrm{amu}$

Hence the molar mass of ibuprofen is $206$amu.

We need to find that How many grams of ibuprofen are in $0.525$mole .

We have to given that the moles of ibuprofen is $0.525$

We know that

localid="1653501154800" $$\begin{gathered} \mathrm{moles}=\frac{\mathrm{weight}\mathrm{in}\mathrm{g}}{\mathrm{molar}\mathrm{mass}\left(\mathrm{amu}\right)} \\ 0.525=\frac{\mathrm{W}\left(\mathrm{g}\right)}{206\left(\mathrm{amu}\right)} \\ \mathrm{W}=108.15\mathrm{g} \end{gathered}$$

We need to find that How many moles of C are in $12.0g$of ibuprofen.

We see the formula $C_{13}{H}_{18}{0}_2$.$1$mol of ibuprofen = $13$mol of$\mathrm{C}$.

So the no of moles in localid="1653459832673" $12g$of ibuprofen is $12/206$.

Moles of ibuprofen are$0.058$moles.

So $0.058$moles of ibuprofen arelocalid="1652672649763" $13×0.058$moles of $C$are $0.75$moles of $\mathrm{C}$.

Hence the no of moles of carbon present in $12$g of ibuprofen are$0.75$.

We need to find that How many moles of ibuprofen contain $1.22x{10}^{23}$atoms of C?

We are given $1.22x{10}^{23}$atoms of carbon.

So

localid="1653501182734" $$\begin{gathered} \mathrm{moles}=\frac{1.22×{10}^{23}}{6×{10}^{23}} \\ \mathrm{moles}=0.20\mathrm{mole} \end{gathered}$$

And we know that

$1$mol of ibuprofen = $13$mol of$\mathrm{C}$.

$0.20$moles of carbon contains = $\frac{\cancel{0.2}}{\cancel{13}}=0.015$moles of ibuprofen.