(a) A flask contains 3.2 g of sulphur dioxide. Calculate the following:(i) The moles of sulphur dioxide present in the flask.(ii) The number of molecules of sulphur dioxide present in the flask.(iii) The volume occupied by 3.2 g of sulphur dioxide at STP. (S = 32, O = 16)(b) The reaction of potassium permanganate (VII) with acidified iron (II) sulphate is given below:2KMnO4 + 10FeSO4 + 8H2SO4 → K2SO4 + 2MnSO4 + 5Fe2(SO4)3 + 8H2OIf 15.8 g of potassium permanganate (VII) was used in the reaction, calculate the mass of iron (II) sulphate used in the above reaction. (K = 39, Mn = 55, Fe = 56, S = 32, O = 16)

(a) A flask contains 3.2 g of sulphur dioxide. Calculate the following

1.	(a) A flask contains 3.2 g of sulphur dioxide. Calculate the following:(i) The moles of sulphur dioxide present in the flask.(ii) The number of molecules of sulphur dioxide present in the flask.(iii) The volume occupied by 3.2 g of sulphur dioxide at STP. (S = 32, O = 16)(b) The reaction of potassium permanganate (VII) with acidified iron (II) sulphate is given below:2KMnO4 + 10FeSO4 + 8H2SO4 → K2SO4 + 2MnSO4 + 5Fe2(SO4)3 + 8H2OIf 15.8 g of potassium permanganate (VII) was used in the reaction, calculate the mass of iron (II) sulphate used in the above reaction. (K = 39, Mn = 55, Fe = 56, S = 32, O = 16)
Answer» (a) A flask contains 3.2 g of sulphur dioxide. Calculate the following: (i) The moles of sulphur dioxide present in the flask. (ii) The number of molecules of sulphur dioxide present in the flask. (iii) The volume occupied by 3.2 g of sulphur dioxide at STP. (S = 32, O = 16) (b) The reaction of potassium permanganate (VII) with acidified iron (II) sulphate is given below: 2KMnO₄ + 10FeSO₄ + 8H₂SO₄ $\overset{}{\to}$ K₂SO₄ + 2MnSO₄ + 5Fe₂(SO₄)₃ + 8H₂O If 15.8 g of potassium permanganate (VII) was used in the reaction, calculate the mass of iron (II) sulphate used in the above reaction. (K = 39, Mn = 55, Fe = 56, S = 32, O = 16)