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Normal melting point: 658 C Normal boiling point: 2467 C
Heat of fusion: 3.95 kJ/g
Heat of vaporization: 10.52 kJ/g Specific heat of solid: 0.902 J/g C

How much energy must be applied to 12 moles of solid aluminum at 72 C to a liquid at 658 C?

Respuesta :

ashimasood1990
{  12 mol  *  27 g / mol * 0.902 j/gdeg C* ( 658 -72 ) deg C  +  12   *   27  * 3.95 }
quantity of energy required to heat  12 mol of aluminium for 72 deg C to its melting point  658  C

so energy applied is   1451 057 . 33  J

 
xero099

Answer:

[tex]Q = 1450089.956\,J[/tex]

Explanation:

The amount of heat required to melt the aluminium is the sum of latent and sensible heats:

[tex]Q = Q_{lat} + Q_{sen}[/tex]

[tex]Q = \left(12\,mol\right)\cdot \left(26.982\,\frac{g}{mol} \right)\cdot \left[\left(0.902\,\frac{J}{g\cdot ^{\textdegree}C} \right)\cdot (658\,^{\textdegree}C - 72\,^{\textdegree}C) + 3950\,\frac{J}{g} \right][/tex]

[tex]Q = 1450089.956\,J[/tex]

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