Question

 A sulfuric acid solution containing 551.5 g of H₂SO₄ per liter of solution has a density of 1.33 g/cm³. Calculate the molality of H₂SO₄ in this

 solution.

 b) The partial vapour pressure of Acetonitrile (1)/ Butanol (2) was measure at 333.15 K with the following results;

 Table 1: Partial vapour pressure data at different mole fraction of Acetonitrile.

 i) Plot a P-y diagram for the Table 1. Prove that the mixture conforms to Roults' Law for the benzene in large excess.

 ii) Determine the Henry's Law constant.

Answer 1

PART 1:

Given that, 1 liter of solution contains 551.5 g of H₂SO₄.

We have molar mass of H₂SO₄, M= 98.079 g/mol.

Therefore no.of moles of H₂SO₄ in 1 liter of solution is given by:

Density of solution = 1.33 g/cm³= 1.33 kg/L.

Therefore, Molality of the solution is given by,

m-molal.

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