A certain substance X condenses at a temperature of 120.7 degree C. But if a 500, g sample of X is prepared with 55.4 g of urea (NH_2)_2 CO) dissolved in it, the sample is found to have a condensation point of 125.2 degree C instead. Calculate the molal boiling point elevation constant K_b of X. Round your answer to 2 significant digits.

The molal boiling point elevation constant of X is

Explanation:

Formula used for Elevation in boiling point :

or,

where,

= boiling point constant  = ?

m = molality

= mass of solute (urea) = 55.4 g

= mass of solvent  X =  500 g

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

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

Thus the molal boiling point elevation constant of X is

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atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer