Question

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?

Answer 1

`Q = 1450089.956\,J`

Step-by-step explanation:

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

`Q = Q_(lat) + Q_(sen)`

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

`Q = 1450089.956\,J`

Answer 2

{ 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