A flask contains 3.2 g of sulphur dioxide. Calculate the followings:

i) The number of molecules of sulphur dioxide at STP.

ii) The volume occupied by 3.2 g of sulphur dioxide at STP.

(S = 32, O = 16)

A- flask contains 3.2 g of sulphur dioxide. Calculate the following (i) the moles of sulphur dioxide present in the flash (ii) the number of molecules of sulphur dioxide present in the flask.

(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) A n experiment showed that in a lead chloride solution 6.21 g of lead is combined with 4.26 g of chlorine. What is the empirical formula of this chloride?
(Pb = 2107; Cl = 35.5).

(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)

A flask contains 3.2 g of sulphur dioxide. Calculate the following :

(a) The moles of sulphur dioxide present in the flask.

(b) The number of molecules of sulphur dioxide present in the flask.

(c) The volume occupied by 3.2 g sulphur dioxide at S.T.P.

A flask conntains 3.2g of sulphur dioxide calculate the following

1.the moles of sulphur dioxide present inthe flask

2.the number of molecules of sulphurdioxide present in the flask

3 the volume occupied by 3.2g of sulphur dioxide at s.t.p[s=32,o=16]