The melting point of aluminum is 660°c, its latent heat of fusion is 4.00 × 105 j/kg, and its specific heat is 900j/kg ∙ k. how much heat must be added to 500 g of aluminum originally at 27°c to completely melt it?

457859J

Explanation:

The parameters given in this question are;

Melting point = 600 °C + 273 = 873 (Converting to kelvin)

Latent heat of fusion = 4.00 × 105 J/kg

Specific heat of capacity (C) = 900J/kg ∙ K

Mass = 500g /1000 = 0.5kg (Converting to Kg)

Initial temperature = 27 + 273 = 300K (Converting to kelvin)

How much heat required to melt it?

To solve this problem, you'll need the formula that relates heat energy to mass and heat of fusion, and heat capacity.

This question is two parts.

We have to calculate how much heat would be required to raise its temperature from 27 to 660 (melting point) and then heat required to melt it.

Heat required to raise its temperature (H1)

H1 = mCθ

θ = T2 - T1 = 873 -  300 = 573K

H1 = 0.5 * 900 * 573

H1 = 257850J

Heat required to melt (H2)

H2 = mL

H2 = 0.5 * 4.00 × 10^5

H2 = 200000J

Total amount of heat required = H1 + H2 = 257859 + 200000

= 457859J

43.452

step-by-step explanation:

284 times .153 = 43.452

the answer is b. dilution