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a. How much energy do you need to transfer to raise the temperature of 150 $\mathrm{g}$ of aluminum from $20^{\circ} \mathrm{C}$ to its melting point?b. How much energy do you need to transfer to melt 150 $\mathrm{g}$ of aluminum?

a) 20128.5 $\mathrm{cal}$b) 14175 $\mathrm{cal}$

Chemistry 102

Chemistry 101

Chapter 18

Observing Energy

Section 6

Heat and Phase Changes

Thermodynamics

Thermochemistry

University of Central Florida

University of Toronto

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Question eight takes into account something learned in this section and also the previous section. First, you're asked to calculate the amount of heat that is required to raise the temperature of aluminum from 20 degrees Celsius to its melting point. This is using the traditional heat equation that was provided in the previous section, where heat is equal to the specific keep capacity of aluminum multiplied by its mass multiplied by its change in temperature. So you'll need to go back to the previous section and look up the specific heat of aluminum. It's point to one calories per gram degree. Celsius will multiply that by the mass 150 g and then multiply that by the change in temperature. The final temperature, which is the melting point of aluminum, which you will look up in the table in this section 659 degrees Celsius, minus the initial temperature 20 degrees Celsius. That then gives us ah heat of 20,100 calories. Now that it it is at its melting point. How much heat is required to melt? 150 g? This then refers to what you learned in this section, where you simply use the heat of fusion to convert the grams of aluminum into the calories of aluminum required to melt it at its melting point, which is three. Heat of fusion of aluminum is 94.5 calories per gram. This then gives us a value of 14,200 calories.

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