Aluminum has a Latent Heat of Fusion of 94.6 calories/gram and a Specific Heat of 0.214 cal/g C. The melting point of Aluminum is 660 C. How much heat would be needed to raise the temperature of 860 grams of Aluminum from 554.4 C to 1379.4 C?
To solve this problem, we need to calculate the amount of heat required to raise the temperature of the aluminum from 554.4°C to its melting point, and then add the heat required to melt the aluminum at its melting point, and finally calculate the heat required to raise the temperature of the Aluminum from its melting point to 1379.4°C.
Let's break down the steps:
Step 1: Calculate the heat required to raise the temperature from 554.4°C to the melting point of Aluminum (660°C).
We can use the equation: Q = m * c * ΔT, where Q is the heat, m is the mass, c is the specific heat, and ΔT is the change in temperature.
Q1 = m * c * ΔT1
Q1 = 860 g * 0.214 cal/g°C * (660°C - 554.4°C)
Step 2: Calculate the heat required to melt the Aluminum.
We can use the equation: Q = m * Latent Heat of Fusion
Q2 = m * Latent Heat of Fusion
Q2 = 860 g * 94.6 cal/g
Step 3: Calculate the heat required to raise the temperature from the melting point of Aluminum to 1379.4°C.
We can use the equation: Q = m * c * ΔT
Q3 = m * c * ΔT3
Q3 = 860 g * 0.214 cal/g°C * (1379.4°C - 660°C)
To get the total heat required, we add Q1, Q2, and Q3.
Total heat = Q1 + Q2 + Q3
Now, you can substitute the values into the equations and calculate the answers.