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Solutions

Question

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Ethylene glycol (molar mass = 62 g mol^–1) is a common automobile auto freeze. Calculate the freezing point of a solution containing 12.4 g of this substance in 100 g of water. Would it be advisable to keep the substance in the car radiator during summer?

Solution

Answer:

W_b = 12.4
n_B= 62g/mol
W_A = 100g

k_{f} for water = 1.86 K kg / mol k_{b} for water = 0.512 K kg / mol

∆ T_{f} = \frac{k_{f} \times 1000 \times W_{B}}{W_{A} \times n_{B}}

or

∆ T_{f} = \frac{1.86 \times 1000 \times 12.4}{100 \times 62} = 3.72 K

Freezing point of the solution
= 273.15 - 3.72 = 269.43K.

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