# Solid iron reacts with sulfuric acid to produce iron (ll) sulfate and hydrogen gas. If 655 mL gas are collected at STP, how many grams of iron (II) sulfate are also produced?

$F e \left(s\right) + {H}_{2} S {O}_{4} \left(a q\right) \rightarrow F e S {O}_{4} \left(a q\right) + {H}_{2} \left(g\right) \uparrow$
It is a fact that at STP, 1 mole of ideal gas (whose behaviour should approximate) has a volume of $22.4$ $L$.
We have $0.655$ $L$ produced by the reaction; i.e. $\frac{0.655 \cdot \cancel{L}}{22.4 \cdot \cancel{L} \cdot m o {l}^{-} 1}$ $=$ $0.292$ $m o l$.
By stoichiometry there must have been $0.292$ $m o l$ $\times$ $151.9 \cdot g \cdot m o {l}^{-} 1$ $=$ ??g $F e S {O}_{4}$.