Question

the molal elevation constant of water is 0.56 K kg Mol .the boiling point of a solution made by dissolving 6.0g urea in 200g of water is

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Answer 1

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Answer 2

The boiling point of a solution made by dissolving 6.0g urea in 200g of water is $100.28^0C$

Explanation:

$T_b-T^o_b=i\times k_b\times \frac{w_2\times 1000}{M_2\times w_1}$

where,

$T_b$ = boiling point of solution = ?

$T^o_b$ = boiling point of water= $100^oC$

$k_b$ = boiling point constant of water = $0.56K/kgmol$

m = molality

i = Van't Hoff factor = 1 (for non-electrolyte)

$w_2$ = mass of solute (urea) = 6.0 g

$w_1$ = mass of solvent (water) = 200 g

$M_2$ = molar mass of solute (urea) = 60 g/mol

Now put all the given values in the above formula, we get:

$(T-b-100)^oC=1\times (0.56K/m)\times \frac{(6.0g)\times 1000}{60\times (200g)}$

$T_b=100.28^0C$

Therefore, the boiling point of the solution is $100.28^0C$

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