[Devils advocate]

How many dm^3 of H₂S  do you get after 1kg of 97% FeS reacts with HCl?

It seems relatively easy, but I don't know how to solve it.
Edit: STP and stoichiometric amount of HCl

[chenbeier]

1. Develop the chemical equation
2. Calculate the 100% mass of FeS
3. Change this to the mole
4. Check with the chemical equation how many mol H₂S correspond
5. Change this with the ideal gas equation  or by using the molar volume to the volume.

NOW ITS YOUR TURN

[AWK]

There is a lack of data for H2S - pressure, temperature, or STP and information on the amount of HCl used (specific or stoichiometric amount or excess).

[chenbeier]

HCl in excess and STP.

[MNIO]

Anytime you get a problem in "stoichiometry".. that is.. how much of this reacts with our how much of that is produced or what is the limiting reagent or what is yield or % yield.. anything like that.. follow these steps
  (1) write a balanced equation
  (2) convert everything given to moles
  (3) determine limiting reagent (there are 3 common ways to do this!)
  (4) convert moles limiting reagent to moles of whatever chemicals you want
  (5) convert moles back to mass (or volume).  This is theoretical mass (or volume)
  (6) % yield = (actual mass recovered / theoretical yield) * 100%

*****
get busy working on those steps!
  where's your balanced equation?
  where's step (2)?
        hint..
           1kg sample*(0.97kg FeS/kg sample)*(1000g/1kg)*(1 mol FeS/__g FeS)=what?
  which is the LR?
  how do you convert mole FeS to mole H2S?
  how do you convert mole H2S to dm³ H2S @STP?... (step 5)