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Tju [1.3M]
3 years ago
10

Acetic acid has a boiling point of 118.5 C and a boiling point constant of 3.08. What is the boiling point of a 3.20 m solution

of Ca(NO3)2 in acetic acid?
Chemistry
1 answer:
puteri [66]3 years ago
6 0

Answer:

T = 401.356 K (128.356°C)

Explanation:

boiling point:

  • ΔT = K×m = T - T*

∴T: boiling temperature of the solution

∴ T*: boiling temperature of pure solvent = 118.5°C ≅ 391.5 K

∴ K: boiling point constant = 3.08 K.Kg/mol

∴ m: molality [=] mol/Kg = 3.20 m

∴  solvent: acetic acid

∴  solute: Ca(NO3)2

⇒ T = T* + (K)(m)

⇒ T = 391.5 K + ((3.08 K.Kg/mol)(3.20 mol/Kg))

⇒ T = 391.5 K + 9.856 K

⇒ T = 401.356 K

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Answer : The reaction rate at 3^oC,24^oC,40^oC\text{ and }65^oC are 36mg/L/sec,142mg/L/sec,190mg/L/sec\text{ and }352mg/L/sec

Solution : Given,

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\text{Reaction rate}=\frac{\text{Mass of tablet}/\text{Volume of water}}{\text{Reaction time}}

Now we have to calculate the reaction rate at different temperatures and reaction time.

\text{Reaction rate at }3^oC=\frac{1000mg/0.200L}{138.5sec}=\frac{5000mg/L}{138.5sec}=36mg/L/sec

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3 years ago
Read 2 more answers
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