Question

How much heat energy is required to melt 25.0 g of Aluminum at its melting point, 658​°​C? (The H​f of Al is 94.4 joules/gram)

Answer 1

2360 joules of heat energy are required to melt 25.0 g of aluminum at its melting point. This is calculated using the heat of fusion for aluminum which is 94.4 joules/gram.

Step-by-step explanation:

To calculate the heat energy required to melt 25.0 g of aluminum at its melting point, we can use the heat of fusion (Hf) for aluminum. The heat of fusion is the amount of heat required to convert a substance from the solid phase to the liquid phase without changing its temperature. Since the heat of fusion (Hf) of aluminum is 94.4 joules/gram, the calculation is straightforward.

The formula to calculate the heat energy (Q) required for the phase change is:

Q = mass (m) × heat of fusion (Hf)

For 25.0 g of aluminum, the calculation would be:

Q = 25.0 g × 94.4 J/g

Q = 2360 joules

Therefore, 2360 joules of heat energy is required to melt 25.0 g of aluminum at its melting point of 658°C.

Answer 2

2360J

Step-by-step explanation:

Given parameters:

Mass of aluminum = 25g

Melting point = 658°C

Latent heat of melting = 94.4j/g

Unknown:

Amount of heat require for melting = ?

Solution:

The amount of heat required for this melting will be the product of the mass of the aluminum and the latent heat of melting;

H = m L

m is the mass

L is the latent heat of melting

Insert the parameters and solve;

H = 25 x 94.4 = 2360J