Question

How many moles of H2SO4 are required for oxidizing 1520g of 37.5% pure FeSO4 to ferric form using 1MKMng: {Mwt of Fe = 56}​

Answer 1

Answer:

I am not pretty sure with this answer can you please comment the answer.

Answer 2

Answer:

2KMnO4+10FeSO4+8H2SO4→K2SO4+2MnSO4+5Fe2(SO4)3+8H2O

∴  2 moles KMnO4 react with 10 moles of FeSO4

∴  1 mol of KMnO4 will react with 5 moles of FeSO4