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.
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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A sulfuric acid solution containing 551.5 g of H2SO4 per liter of solution has a density of 1.33 g/cm3
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