Respuesta :
Answer: The mass of [tex]FeO[/tex] required is 14.37 g
Explanation:
Molarity is calculated by using the equation:
[tex]\text{Molarity}=\frac{\text{Moles}}{\text{Volume}}[/tex] ......(1)
We are given:
Molarity of iron (II) sulfate = 1 M
Volume of solution = 200 mL = 0.200 L (Conversion factor: 1 L = 1000 mL)
Putting values in equation 1, we get:
[tex]\text{Moles of }FeSO_4=(1mol/L\times 0.200L)=0.200mol[/tex]
The chemical equation for the reaction of FeO with sulfuric acid follows:
[tex]FeO+H_2SO_4\rightarrow FeSO_4+H_2O[/tex]
By stoichiometry of the reaction:
If 1 mole of iron (II) sulfate is produced by 1 mole of FeO
So, 0.200 moles of iron (II) sulfate will produce = [tex]\frac{1}{1}\times 0.200=0.200mol[/tex] of FeO
The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
We know, molar mass of [tex]FeO[/tex] = 71.84 g/mol
Putting values in above equation, we get:
[tex]\text{Mass of }FeO=(0.200mol\times 71.84g/mol)=14.37g[/tex]
Hence, the mass of [tex]FeO[/tex] required is 14.37 g
