Iron weighing 14 g was fused with sulfur weighing 4.8 g, and hcl was added to the resulting mixture.

Iron weighing 14 g was fused with sulfur weighing 4.8 g, and hcl was added to the resulting mixture. What gases are released and what are their volumes?

We write down the equation of reactions.
Fe + S = FeS.
We find the amount of the substance iron and sulfur. We use the following formula.
n = m / M.
We calculate the molar mass of iron and sulfur.
M (Fe) = 56 g / mol.
M (S) = 32 g / mol.
We find the amount of substance.
n (Fe) = 14 g / 56 g / mol = 0.25 mol.
n (S) = 4.8 g / 32 g / mol = 0.15 mol.
This means that iron is in excess, which means we will count by sulfur.
We write down the uranium of reactions.
0.15 mol S = 0.15 mol FeS.
FeS + 2 HCL = FeCl 2 + H2S.
Next, we find the amount of hydrogen sulfide substance by the reaction equation.
0.15 mol FeS – х mol H2S
1 mol FeS – 1 mol H2S
Hence, n (H2S) = 0.15 mol.
Next, we find the volume.
n = V / Vm.
V = n × Vm = 0.15 mol × 22.4 L / mol = 3.36 L.
Answer: hydrogen sulfide H2S gas with a volume of 3.36 liters will be released.