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babunello [35]
3 years ago
8

The freezing point of a solution prepared by dissolving 150 × 10–3 g of caffeine in 10.0 g of camphor is lower by 3.07°C than th

at of pure camphor (Kf = 39.7°C/m). What is the molar mass of caffeine?
Physics
1 answer:
Finger [1]3 years ago
6 0

Answer:

Molar Mass=193.9738 g/mol

Molar Mass≅194g/mol

Explanation:

Consider the formula:

m=ΔT/K_{f}

where:

ΔT is freezing point depression

K_{f} is freezing point depression constant

m is the morality=(moles of solute/kg of solvent)

Now:

m=\frac{3.07}{39.7}

m=0.07733 moles of solute/kg of solvent

Now:

0.07733 (moles of solute/kg of solvent) *0.010 kg of solvent

7.733*10^{-4} moles of solute(Caffeine)

Molar mass = Mass of solute/moles of solute

Molar Mass=\frac{150*10^-3}{7.733*10^{-4} }

Molar Mass=193.9738 g/mol

Molar Mass≅194g/mol

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