Lead(II) sulfide dissolves in excess nitric acid according to the equation below. Calculate the volume of $\ce{NO{(g)}}$ at $\pu{27 ^\circ C}$ and $\pu{1.10 atm}$ produced from $\pu{4.7 g}$ of $\ce{PbS(s)}$.
$$\ce{3PbS{(s)} + 2NO3–{(aq)} + 8H+{(aq)} -> 3Pb^2+{(aq)} + 3S{(s)} + 2NO{(g)} + 4H2O{(l)}}$$
a) $\pu{0.29 L}$
b) $\pu{0.44 L}$
c) $\pu{0.66 L}$
d) $\pu{30 L}$
e) $\pu{45 L}$
I used the ideal gas formula and converted the mass of $\ce{PbS}$ into number of moles of $\ce{PbS}$ however got the answer b) $\pu{0.44 L}$ which is incorrect. The correct answer is a) however I am unsure about. Why this is?