Expansion of ideal gas in isothermic conditions

I'm doing this problem and I get a different value than the answer in a book. I'm not sure if the book is wrong or me. 



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> At a constant temperature of $298~\mathrm{K}$, calculate $\Delta S\_{\mathrm{sys}}$ and $\Delta S\_{\mathrm{univ}}$ for the free expansion of $3.0~\mathrm{L}$ of an ideal gas at $1.0~\mathrm{atm}$ to $11.0~\mathrm{L}$.
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My solution
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Firstly, I calculated the moles of gas $n$:


$$\begin{align}
n &= \frac{PV}{RT} \\
&= \frac{(1~\mathrm{atm}) \cdot (3.0~\mathrm{L})}{(0.0821~\mathrm{L~atm~mol^{-1}~K^{-1}})\cdot(298~\mathrm{K})} \\
&= 0.1226~\mathrm{mol}
\end{align}$$


Secondly, I used this to calculate $\Delta S$:


$$\begin{align}
\Delta S &= nR \ln{\frac{V\_2}{V\_1}} \\
&= (0.1226~\mathrm{mol}) \cdot (0.0821~\mathrm{L~atm~mol^{-1}~K^{-1}}) \cdot \ln{\left(\frac{11.0~\mathrm{L}}{3.0~\mathrm{L}}\right)} \\
&= 0.0130~\mathrm{L~atm~K^{-1}}
\end{align}$$


However, the answer in the book is $0.027~\mathrm{L~atm~K^{-1}}$. I'm not sure if that's an error. 


