The reaction of potassium permanganate (VII) with acidified iron(II) sulphate is given below:

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)

Q. The reaction of potassium permanganate with acidified iron [II] sulphate is given below :- $2KMn{O}_4+10FeS{O}_4+8H_{2}S{O}_4\to K_{2}S{O}_4+2MnS{O}_4+5F{e}_2(S{O}_4{)}_3+8H_{2}O$
If $15.8$ g of potassium permanganate was used in the reaction, calculate the mass of iron [II] sulphate used in the above reaction.
[Molecular Weight of $K=39,Mn=55,Fe=56,S=32,O=16$ g/mole]

Q.

(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 $\stackrel{}{\to }$ 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)

Q. The reaction, is an example of reaction of:

Q. Identify the correctly balanced redox reaction using ion-electron method.
$FeS{O}_4+KMn{O}_4+H_{2}S{O}_4\to F{e}_2(S{O}_4{)}_3+MnS{O}_4+H_{2}O+K_{2}S{O}_4$

Q.

Calculate the relative molecular masses of (Use K = 39, Cl = 35.5, O = 16, C = 12, H = 1, Na = 23, N = 14, S = 32)
(a) potassium chlorate
(b) sodium acetate
(c) chloroform
(d) ammonium sulphate