Explanation:
[tex]molar \: mass \: of \: iron = 56 \: g \\ 56 \: g\: are \: weighed \: by \: 1 \: mole \: of \: iron \\ 595 \: g \: will \: be \: weighed \: by \: ( \frac{595}{56} ) \: moles \\ = 10.625 \: moles \: of \: iron \\ from \: equation : \\ 1 \: mole \: of \: iron \: is \: formed \: by \: 1 \: mole \: of \: hydrogen \\ 10.625 \: moles \: will \: be \: produced \: by \: (10.625 \times 1) \: moles \\ = 10.625 \: moles \: of \: hydrogen \\ at \: s.t.p : \\ 1 \: mole \: = \: 22.4 \: litres \\ 10.625 \: moles \: = (22.4 \times 10.625) \\ = 238 \: litres \\ \\ or \: at \: r.t.p : \\ 1 \: mole \: = 24 \: litres \\ 10.625 \: moles \: = \: (10.625 \times 24) \\ = 255 \: litres[/tex]
