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3 years ago

What is the thermal energy needed to completely melt 9.60 mol of ice at 0.0 C

Chemistry

2 answers:

jeka57 [31]3 years ago

5 0

Answer:

57.792 kJ

Explanation:

Molar enthalpy of fusion of the substance is defined as the energy required to convert the substance in solid state, at its melting point to liquid state at constant pressure and no change in temperature.

For example the energy required to convert 1 mole of water (ice) at 0°C to 1 mole of water (liquid) at 0°C is 6.02 kJ/mol.

Thus, thermal energy required to convert 9.60 moles of ice is 6.02×9.60 kJ = 57.792 kJ

inysia [295]3 years ago

4 0

The thermal energy needed to completely melt 9.60 mole of ice at 0.0 C is 57.8 Kj

Explanation
ice melt to form water

The molar heat of fusion for water is 6.02 Kj/mol
Thermal energy = moles x molar heat of fussion for water

=9.6 mol x6.02 kj/mol =57.8 Kj

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Answer: The freezing point and boiling point of the solution are $-6.6^0C$ and $101.8^0C$ respectively.

Explanation:

Depression in freezing point:

$T_f^0-T^f=i\times k_f\times \frac{w_2\times 1000}{M_2\times w_1}$

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$T_f$ = freezing point of solution = ?

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Now put all the given values in the above formula, we get:

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$k_b$ = boiling point constant of water = $0.52^0C/m$

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$w_2$ = mass of solute (ethylene glycol) = 21.4 g

$w_1$ = mass of solvent (water) = $density\times volume=1.00g/ml\times 97.6ml=97.6g$

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$(T_b-100)^0C=1\times (0.52^0C/m)\times \frac{(21.4g)\times 1000}{97.6g\times (62g/mol)}$

$T_b=101.8^0C$

Thus the boiling point of the solution is $101.8^0C$

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