73. calculate the number of moles and molecules present in sulphur dioxide obtained by combustion of 6.4 * 10-2 kilogram of sulphur

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Q. Calculate the number of moles of

6.022 \times 10^{23}

molecules of sulphur dioxide.

Q. Calculate the number of oxygen atoms in 0.1 mole of sulphur dioxide molecules.

(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).

The sulphur dioxide obtained by the combustion of 8 g of sulphur is passed into Bromine water. The solution is then treated with barium chloride solution. The amount of barium sulphate formed is

(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)

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