Answer to Question #182018 in General Chemistry for Sally

Question

Calculate the amount of energy and KJ required to melt a 16.2 g aluminum pop can assume that the initial temperature of the aluminum it’s 20°C give your answer to two decimal places.

aditional info:

molar heat of fusion of Al=10.7 kj/mol

melting point of aluminum=660°c

heat capacity of Al=0.900j/g°c

Answer 1

Ans:-

Mole$=\dfrac{16.2}{26.98154}g/mol=0.600 mol$

$\Delta H=(20\degree C\to660\degree C) +(melt)\\ \Delta H=(mc\Delta T)+(n\Delta Hfus)\\ \Delta H=(16.2g)(0.900J/g\degree C)(640\degree C)+(0.600 mol)(10.7kJ/mol)$

$\Delta H=9331.2J+6.42kJ\\ \Delta H=9.33kJ+6.42kJ\\ \Delta H=15.8kJ$