Answer:
100.98 g/mol
Explanation:
Solution:
1) Determine temperature change:
48.1 - 35.8 = 12.3 °C
2) Determine how many moles of the compound dissolved:
Δt = i Kf m
1.674 °C = (1) (9.8 °C kg mol¯1) (x / 0.010009 kg)
9.8 °C = (979.12 °C mol¯1) (x)
x = 0.010009 mol
3) Determine molecular weight:
1.0108 g / 0.010009 mol = 100.98 g/mol
The molecular weight of the unknown compound is 100.98 g/mol.
It is the difference between initial and final temperatures.
[tex]\triangle t = 48.1 - 35.8 = 12.3^oC[/tex]
[tex]\triangle t = i* K_f *m\\\\1.674^oC = (1) (9.8^oC kg mol^{-1}) \frac{x}{0.010009 kg}\\\\ 9.8^oC = (979.12^oC mol^{-1}) (x)\\\\x = 0.010009 mol[/tex]
It is given by mass over number of moles.
[tex]\frac{ 1.0108 g }{0.010009 mol} = 100.98 g/mol[/tex]
Thus, the molecular weight of the unknown compound is 100.98 g/mol.
Find more information about Molecular weight here:
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