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An 21.9-gg ice cube at 0?C?C is placed onto a 355-gg block of aluminum. Calculate the temperature change of the aluminum upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from aluminum. The specific heat capacity of aluminum is 0.903 J/g??CJ/g??C and the heat of fusion for water is 6.02 kJ/molkJ/mol.

Hint:

To calculate the temperature change of the aluminum upon the complete melting of the ice first you need to know how much energy was required to convert the ice to liquid water. Use the equation:

q=n?Hfus=?fus

where n is the number of moles of ice and ?Hfus is the heat of fusion.

qice?ice = |
7320 |
JJ |

To calculate the temperature change of the aluminum upon the complete melting of the ice, we first need to find how much energy is required to convert