In the aqueous solution of H2SO4 its mole fraction is 0.2 then closest value of molality or solution is
a)13.9 b)9.8
c)10.2 d)11.2
13.89
To find the closest value of molality or solution, we need to understand the relationship between mole fraction and molality in a solution.
Mole fraction is the ratio of the moles of a solute to the total moles of solute and solvent in a solution. It is calculated using the formula:
Mole fraction of solute (Xsolute) = moles of solute / (moles of solute + moles of solvent)
Molality, on the other hand, is the ratio of the moles of solute to the mass of the solvent in kilograms. It is calculated using the formula:
Molality (m) = moles of solute / mass of solvent (in kg)
In the given problem, the mole fraction of H2SO4 in the aqueous solution is 0.2. This means that the moles of H2SO4 are 0.2 times the sum of the moles of H2SO4 and moles of water in the solution.
Let's assume the moles of H2SO4 is x and the moles of water is y. From the mole fraction definition:
0.2 = x / (x + y)
To find the relation between mole fraction and molality, we need the molar mass of H2SO4. The molar mass of H2SO4 is approximately:
Molar mass of H2SO4 = (2 * atomic mass of H) + (1 * atomic mass of S) + (4 * atomic mass of O)
= (2 * 1.008) + 32.07 + (4 * 16.00)
≈ 98.09 g/mol
Now, let's find the relation between mole fraction and molality. The molality (m) is given by:
m = x / (mass of water in kg)
To calculate the mass of water in kg, we need to know the density of the solution or the volume of the solution. Unfortunately, this information is not provided in the question. Therefore, we cannot directly calculate the value of molality (m).
Considering the given options (a) 13.9, (b) 9.8, (c) 10.2, and (d) 11.2, none of them can be determined without additional information.
In conclusion, the answer cannot be determined without information about the density of the solution or the volume of the solution.