Calculate the volume of gas that will be released when an excess of iron (II) sulfide is applied to 500 g of a 12% sulfuric acid solution.
November 12, 2020
1) Let’s compose the reaction equation:
FeS + H2SO4 = FeSO4 + H2S ↑
2) Calculate the mass and amount of the sulfuric acid substance contained in the solution:
m (H2SO4) = (m (solution) ∙ ω) / 100% = (500 ∙ 12) / 100 = 60 g;
n (H2SO4) = m (H2SO4) / M (H2SO4) = 60/98 = 0.61 mol.
3) Determine the volume of hydrogen sulfide:
according to the reaction equation
n (H2S) = n (H2SO4) = 0.61 mol;
V (H2S) = n (H2S) ∙ Vm = 0.61 ∙ 22.4 = 13.66 l.
Answer: 13.66 liters.
Remember: The process of learning a person lasts a lifetime. The value of the same knowledge for different people may be different, it is determined by their individual characteristics and needs. Therefore, knowledge is always needed at any age and position.