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densk [106]
3 years ago
11

A solution made by dissolving 14.2g of sucrose in 100g water exhibits a freezing point depression of 0.77 degrees. Calculate the

molar mass of sucrose
Chemistry
1 answer:
Nataly [62]3 years ago
5 0

For the purpose we have to know following equation for freezing point depression:


ΔTf=Kf*b


and that Kf of water is 1.86°C/m.


From the formula we can determine molality (b):


b=Δtf/Kf=0.77/1.86= 0.414 mole/kg


Now when we know molality, we can calculate mass of sucrose in solution:


b=n/m(H20)   =>  n(sucrose)=b*m(H20) = 0.414 mole/kg *0.1 kg = 0.0414 mole


Finally, we can determine the molar mass of sucrose:


M=m/n=14.2/0.0414= 343g/mole

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Kp = 0.022

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<em>Full question: ...With 2.3 atm of ammonia gas at 32. °C. He then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 0.69 atm. </em>

<em />

The equilibrium of ammonia occurs as follows:

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<em />

As initial pressure of ammonia is 2.3atm, its equilibrium concentration will be:

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<em>Where X represents reaction coordinate</em>

<em />

Thus, pressure of hydrogen and nitrogen is:

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As partial pressure of hydrogen is 0.69atm:

3X = 0.69

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<h3>Kp = 0.022</h3>
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